text:
1Thermodynamic statement
1.1Explicit statement
1.1.1'Feedback' variable change blocked or permitted
1.1.2'Driving' variable changed or unchanged
2Other statements
3Chemistry
3.1Effect of change in concentration
3.2Effect of change in temperature
3.3Effect of change in pressure
3.4Effect of change in volume
3.5Effect of adding an inert gas
3.6Effect of a catalyst
4General statement of Le Chatelier's principle
5General statements related to Le Chatelier's principle
6Related system concepts
7Economics
10Bibliography of cited sources
Le Chatelier's principle
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Principle to predict effects of a change in conditions on a chemical equilibrium
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Le Chatelier's principle (pronounced UK: /lə ʃæˈtɛljeɪ/ or US: /ˈʃɑːtəljeɪ/), also called Chatelier's principle (or the Equilibrium Law),[1][2] is a principle of chemistry used to predict the effect of a change in conditions on chemical equilibria. The principle is named after French chemist Henry Louis Le Chatelier, and sometimes also credited to Karl Ferdinand Braun, who discovered it independently. It can be stated as:
When a simple system in thermodynamic equilibrium is subjected to a change in concentration, temperature, volume, or pressure, (1) the system changes to a new equilibrium, and (2) this change partly counteracts the applied change.
Phenomena in apparent contradiction to Le Chatelier's principle can also arise in systems of simultaneous equilibrium (see response reactions).
Le Chatelier's principle is sometimes alluded to in discussions of topics other than thermodynamics.
Thermodynamic statement[edit]
Introduction The following thermodynamic statement is abstract, in general terms, but, for introduction, it may help the reader to bear in mind a simple example: A body of gas in a cylinder with a piston has its pressure externally controlled through pressure on the piston. The body of gas starts in a state of internal thermodynamic equilibrium by setting its own volume. The externally controlled pressure is then 'perturbed' by a controlled finite amount, say Δ P , {\displaystyle \Delta P,} and the body of gas sets its own volume again through a change in volume Δ V . {\displaystyle \Delta V.} If the piston and cylinder are insulated so that the gas cannot gain or lose energy as heat, then the Le Chatelier–Braun principle has nothing to say, because, though the temperature of the gas may change, there is available no possibility of 'moderation' or 'feedback'. But if the piston and cylinder walls conduct heat between the body of gas and a closed external 'heat reservoir' of externally controlled temperature and internal energy, then 'moderation' or 'feedback' can occur, or be investigated, through temperature change in, or heat transfer to or from, the body of gas; and the Le Chatelier–Braun principle tells about it.
General scenario The Le Chatelier–Braun principle analyzes the qualitative behaviour of a thermodynamic system when a designated one of its externally controlled state variables, say L , {\displaystyle L,} changes by an amount Δ L , {\displaystyle \Delta L,} the 'driving change', causing a change δ i M , {\displaystyle \delta _{\mathrm {i} }M,} the 'response of prime interest', in its conjugate state variable M , {\displaystyle M,} all other externally controlled state variables remaining constant. The response illustrates 'negative feedback' and so is 'moderated' in ways evident in two related thermodynamic equilibria. Obviously, one of L , {\displaystyle L,} M {\displaystyle M} has to be intensive, the other extensive. Also as a necessary part of the scenario, there is a designated auxiliary 'moderating' or 'feedback' state variable X {\displaystyle X} , with its conjugate state variable Y . {\displaystyle Y.} For this to be of interest, the 'moderating' variable X {\displaystyle X} must undergo a change Δ X ≠ 0 {\displaystyle \Delta X\neq 0} or δ X ≠ 0 {\displaystyle \delta X\neq 0} in some part of the experimental protocol; this can be either by imposition of a change Δ Y {\displaystyle \Delta Y} , or with the holding of Y {\displaystyle Y} constant, written δ Y = 0. {\displaystyle \delta Y=0.} For the principle to hold with full generality, X {\displaystyle X} must be extensive or intensive accordingly as M {\displaystyle M} is so. Obviously, to give this scenario physical meaning, the 'driving' variable and the 'moderating' or 'feedback' variable must be subject to separate independent experimental controls and measurements.
Explicit statement[edit]
The principle can be stated in two ways, formally different, but substantially equivalent, and, in a sense, mutually 'reciprocal'. The two ways illustrate the Maxwell relations, and the stability of thermodynamic equilibrium according to the second law of thermodynamics, evident as the spread of energy amongst the state variables of the system in response to an imposed change.
The two ways of statement share an 'index' experimental protocol (denoted P i ) , {\displaystyle {\mathcal {P}}_{\mathrm {i} }),} that may be described as 'changed driver, feedback permitted'. Along with the driver change Δ L , {\displaystyle \Delta L,} it imposes a constant Y , {\displaystyle Y,} with δ i Y = 0 , {\displaystyle \delta _{\mathrm {i} }Y=0,} and allows the uncontrolled 'moderating' variable response δ i X , {\displaystyle \delta _{\mathrm {i} }X,} along with the 'index' response of interest δ i M . {\displaystyle \delta _{\mathrm {i} }M.}
The two ways of statement differ in their respective compared protocols. One way posits a 'changed driver, no feedback' protocol (denoted P n ) . {\displaystyle {\mathcal {P}}_{\mathrm {n} }).} The other way posits a 'fixed driver, imposed feedback' protocol (denoted P f . {\displaystyle {\mathcal {P}}_{\mathrm {f} }.} )
'Feedback' variable change blocked or permitted[edit]
This way compares P i {\displaystyle {\mathcal {P}}_{\mathrm {i} }} with P n , {\displaystyle {\mathcal {P}}_{\mathrm {n} },} to compare the effects of the imposed the change Δ L {\displaystyle \Delta L} with and without feedback. The protocol P n {\displaystyle {\mathcal {P}}_{\mathrm {n} }} prevents 'feedback' by enforcing that Δ X = 0 {\displaystyle \Delta X=0} through an adjustment Δ Y , {\displaystyle \Delta Y,} and it observes the 'no-feedback' response Δ M . {\displaystyle \Delta M.} Provided that the observed response is indeed that δ i X ≠ 0 , {\displaystyle \delta _{\mathrm {i} }X\neq 0,} then the principle states that | δ i M | < | Δ M | {\displaystyle |\delta _{\mathrm {i} }M|<|\Delta M|} .
In other words, change in the 'moderating' state variable X {\displaystyle X} moderates the effect of the driving change in L {\displaystyle L} on the responding conjugate variable M . {\displaystyle M.} [3][4]
'Driving' variable changed or unchanged[edit]
This way also uses two experimental protocols, P i {\displaystyle {\mathcal {P}}_{\mathrm {i} }} and P f {\displaystyle {\mathcal {P}}_{\mathrm {f} }} , to compare the index effect δ i M {\displaystyle \delta _{\mathrm {i} }M} with the effect δ f M {\displaystyle \delta _{\mathrm {f} }M} of feedback alone. The 'index' protocol P i {\displaystyle {\mathcal {P}}_{\mathrm {i} }} is executed first; the response of prime interest, δ i M , {\displaystyle \delta _{\mathrm {i} }M,} is observed, and the response Δ X {\displaystyle \Delta X} of the 'feedback' variable is also measured. With that knowledge, then the 'fixed driver, feedback imposed' protocol P f {\displaystyle {\mathcal {P}}_{\mathrm {f} }} enforces that Δ L = 0 , {\displaystyle \Delta L=0,} with the driving variable L {\displaystyle L} held fixed; the protocol also, through an adjustment Δ f Y , {\displaystyle \Delta _{\mathrm {f} }Y,} imposes a change Δ X {\displaystyle \Delta X} (learnt from the just previous measurement) in the 'feedback' variable, and measures the change δ f M . {\displaystyle \delta _{\mathrm {f} }M.} Provided that the 'feedback' response is indeed that Δ X ≠ 0 , {\displaystyle \Delta X\neq 0,} then the principle states that the signs of δ i M {\displaystyle \delta _{\mathrm {i} }M} and δ f M {\displaystyle \delta _{\mathrm {f} }M} are opposite.
Again, in other words, change in the 'feedback' state variable X {\displaystyle X} opposes the effect of the driving change in L {\displaystyle L} on the responding conjugate variable M . {\displaystyle M.} [5]
Other statements[edit]
The duration of adjustment depends on the strength of the negative feedback to the initial shock. The principle is typically used to describe closed negative-feedback systems, but applies, in general, to thermodynamically closed and isolated systems in nature, since the second law of thermodynamics ensures that the disequilibrium caused by an instantaneous shock is eventually followed by a new equilibrium.[6]
While well rooted in chemical equilibrium, Le Chatelier's principle can also be used in describing mechanical systems in that a system put under stress will respond in such a way as to reduce or minimize that stress. Moreover, the response will generally be via the mechanism that most easily relieves that stress. Shear pins and other such sacrificial devices are design elements that protect systems against stress applied in undesired manners to relieve it so as to prevent more extensive damage to the entire system, a practical engineering application of Le Chatelier's principle.
Chemistry[edit]
Effect of change in concentration[edit]
Changing the concentration of a chemical will shift the equilibrium to the side that would counter that change in concentration. The chemical system will attempt to partly oppose the change affected to the original state of equilibrium. In turn, the rate of reaction, extent, and yield of products will be altered corresponding to the impact on the system.
This can be illustrated by the equilibrium of carbon monoxide and hydrogen gas, reacting to form methanol.
CO + 2 H2 ⇌ CH3OH
Suppose we were to increase the concentration of CO in the system. Using Le Chatelier's principle, we can predict that the concentration of methanol will increase, decreasing the total change in CO. If we are to add a species to the overall reaction, the reaction will favor the side opposing the addition of the species. Likewise, the subtraction of a species would cause the reaction to "fill the gap" and favor the side where the species was reduced. This observation is supported by the collision theory. As the concentration of CO is increased, the frequency of successful collisions of that reactant would increase also, allowing for an increase in forward reaction, and generation of the product. Even if the desired product is not thermodynamically favored, the end-product can be obtained if it is continuously removed from the solution.
The effect of a change in concentration is often exploited synthetically for condensation reactions (i.e., reactions that extrude water) that are equilibrium processes (e.g., formation of an ester from carboxylic acid and alcohol or an imine from an amine and aldehyde). This can be achieved by physically sequestering water, by adding desiccants like anhydrous magnesium sulfate or molecular sieves, or by continuous removal of water by distillation, often facilitated by a Dean-Stark apparatus.
Effect of change in temperature[edit]
The reversible reaction N2O4(g) ⇌ 2NO2(g) is endothermic, so the equilibrium position can be shifted by changing the temperature.
When heat is added and the temperature increases, the reaction shifts to the right and the flask turns reddish brown due to an increase in NO2. This demonstrates Le Chatelier's principle: the equilibrium shifts in the direction that consumes energy.
When heat is removed and the temperature decreases, the reaction shifts to the left and the flask turns colorless due to an increase in N2O4: again, according to Le Chatelier's principle.
The effect of changing the temperature in the equilibrium can be made clear by 1) incorporating heat as either a reactant or a product, and 2) assuming that an increase in temperature increases the heat content of a system. When the reaction is exothermic (ΔH is negative and energy is released), heat is included as a product, and when the reaction is endothermic (ΔH is positive and energy is consumed), heat is included as a reactant. Hence, whether increasing or decreasing the temperature would favor the forward or the reverse reaction can be determined by applying the same principle as with concentration changes.
Take, for example, the reversible reaction of nitrogen gas with hydrogen gas to form ammonia:
N2(g) + 3 H2(g) ⇌ 2 NH3(g) ΔH = −92 kJ mol−1
Because this reaction is exothermic, it produces heat:
N2(g) + 3 H2(g) ⇌ 2 NH3(g) + heat
If the temperature were increased, the heat content of the system would increase, so the system would consume some of that heat by shifting the equilibrium to the left, thereby producing less ammonia. More ammonia would be produced if the reaction were run at a lower temperature, but a lower temperature also lowers the rate of the process, so, in practice (the Haber process) the temperature is set at a compromise value that allows ammonia to be made at a reasonable rate with an equilibrium concentration that is not too unfavorable.
In exothermic reactions, an increase in temperature decreases the equilibrium constant, K, whereas in endothermic reactions, an increase in temperature increases K.
Le Chatelier's principle applied to changes in concentration or pressure can be understood by giving K a constant value. The effect of temperature on equilibria, however, involves a change in the equilibrium constant. The dependence of K on temperature is determined by the sign of ΔH. The theoretical basis of this dependence is given by the Van 't Hoff equation.
Effect of change in pressure[edit]
The equilibrium concentrations of the products and reactants do not directly depend on the total pressure of the system. They may depend on the partial pressure of the products and reactants, but if the number of moles of gaseous reactants is equal to the number of moles of gaseous products, pressure has no effect on equilibrium.
Changing total pressure by adding an inert gas at constant volume does not affect the equilibrium concentrations (see Effect of adding an inert gas below).
Changing total pressure by changing the volume of the system changes the partial pressures of the products and reactants and can affect the equilibrium concentrations (see §Effect of change in volume below).
Effect of change in volume[edit]
Changing the volume of the system changes the partial pressures of the products and reactants and can affect the equilibrium concentrations. With a pressure increase due to a decrease in volume, the side of the equilibrium with fewer moles is more favorable[7] and with a pressure decrease due to an increase in volume, the side with more moles is more favorable. There is no effect on a reaction where the number of moles of gas is the same on each side of the chemical equation.
Considering the reaction of nitrogen gas with hydrogen gas to form ammonia:
N2 + 3 H24 moles ⇌ 2 NH32 moles ΔH = −92kJ mol−1
Note the number of moles of gas on the left-hand side and the number of moles of gas on the right-hand side. When the volume of the system is changed, the partial pressures of the gases change. If we were to decrease pressure by increasing volume, the equilibrium of the above reaction will shift to the left, because the reactant side has a greater number of moles than does the product side. The system tries to counteract the decrease in partial pressure of gas molecules by shifting to the side that exerts greater pressure. Similarly, if we were to increase pressure by decreasing volume, the equilibrium shifts to the right, counteracting the pressure increase by shifting to the side with fewer moles of gas that exert less pressure. If the volume is increased because there are more moles of gas on the reactant side, this change is more significant in the denominator of the equilibrium constant expression, causing a shift in equilibrium.
Effect of adding an inert gas[edit]
See also: § Effect of change in pressure
An inert gas (or noble gas), such as helium, is one that does not react with other elements or compounds. Adding an inert gas into a gas-phase equilibrium at constant volume does not result in a shift.[7] This is because the addition of a non-reactive gas does not change the equilibrium equation, as the inert gas appears on both sides of the chemical reaction equation. For example, if A and B react to form C and D, but X does not participate in the reaction: a A + b B + x X ↽ − − ⇀ c C + d D + x X {\displaystyle {\ce {{\mathit {a}}A{}+{\mathit {b}}B{}+{\mathit {x}}X<=>{\mathit {c}}C{}+{\mathit {d}}D{}+{\mathit {x}}X}}} . While it is true that the total pressure of the system increases, the total pressure does not have any effect on the equilibrium constant; rather, it is a change in partial pressures that will cause a shift in the equilibrium. If, however, the volume is allowed to increase in the process, the partial pressures of all gases would be decreased resulting in a shift towards the side with the greater number of moles of gas. The shift will never occur on the side with fewer moles of gas. It is also known as Le Chatelier's postulate.
Effect of a catalyst[edit]
A catalyst increases the rate of a reaction without being consumed in the reaction. The use of a catalyst does not affect the position and composition of the equilibrium of a reaction, because both the forward and backward reactions are sped up by the same factor.
For example, consider the Haber process for the synthesis of ammonia (NH3):
N2 + 3 H2 ⇌ 2 NH3
In the above reaction, iron (Fe) and molybdenum (Mo) will function as catalysts if present. They will accelerate any reactions, but they do not affect the state of the equilibrium.
General statement of Le Chatelier's principle[edit]
Le Chatelier's principle refers to states of thermodynamic equilibrium. The latter are stable against perturbations that satisfy certain criteria; this is essential to the definition of thermodynamic equilibrium.
It states that changes in the temperature, pressure, volume, or concentration of a system will result in predictable and opposing changes in the system in order to achieve a new equilibrium state.
For this, a state of thermodynamic equilibrium is most conveniently described through a fundamental relation that specifies a cardinal function of state, of the energy kind, or of the entropy kind, as a function of state variables chosen to fit the thermodynamic operations through which a perturbation is to be applied.[8][9][10]
In theory and, nearly, in some practical scenarios, a body can be in a stationary state with zero macroscopic flows and rates of chemical reaction (for example, when no suitable catalyst is present), yet not in thermodynamic equilibrium, because it is metastable or unstable; then Le Chatelier's principle does not necessarily apply.
General statements related to Le Chatelier's principle[edit]
A body can also be in a stationary state with non-zero rates of flow and chemical reaction; sometimes the word "equilibrium" is used in reference to such states, though by definition they are not thermodynamic equilibria. Sometimes, it is proposed to consider Le Chatelier's principle for such states. For this exercise, rates of flow and of chemical reaction must be considered. Such rates are not supplied by equilibrium thermodynamics. For such states, it has turned out to be difficult or unfeasible to make valid and very general statements that echo Le Chatelier's principle.[11] Prigogine and Defay demonstrate that such a scenario may or may not exhibit moderation, depending upon exactly what conditions are imposed after the perturbation.[12]
Related system concepts[edit]
It is common to treat the principle as a more general observation of systems,[13] such as
When a settled system is disturbed, it will adjust to diminish the change that has been made to it
or, "roughly stated":[13]
Any change in status quo prompts an opposing reaction in the responding system.
The concept of systemic maintenance of a stable steady state despite perturbations has a variety of names, and has been studied in a variety of contexts, chiefly in the natural sciences. In chemistry, the principle is used to manipulate the outcomes of reversible reactions, often to increase their yield. In pharmacology, the binding of ligands to receptors may shift the equilibrium according to Le Chatelier's principle, thereby explaining the diverse phenomena of receptor activation and desensitization.[14] In biology, the concept of homeostasis is different from Le Chatelier's principle, in that homoeostasis is generally maintained by processes of active character, as distinct from the passive or dissipative character of the processes described by Le Chatelier's principle in thermodynamics. In economics, even further from thermodynamics, allusion to the principle is sometimes regarded as helping explain the price equilibrium of efficient economic systems. In some dynamic systems, the end-state cannot be determined from the shock or perturbation.
Economics[edit]
In economics, a similar concept also named after Le Chatelier was introduced by American economist Paul Samuelson in 1947. There the generalized Le Chatelier principle is for a maximum condition of economic equilibrium: Where all unknowns of a function are independently variable, auxiliary constraints—"just-binding" in leaving initial equilibrium unchanged—reduce the response to a parameter change. Thus, factor-demand and commodity-supply elasticities are hypothesized to be lower in the short run than in the long run because of the fixed-cost constraint in the short run.[15]
Since the change of the value of an objective function in a neighbourhood of the maximum position is described by the envelope theorem, Le Chatelier's principle can be shown to be a corollary thereof.[16]
Common-ion effect
Response reactions
^ "Le Chatelier's principle (video)". Khan Academy. Archived from the original on 2021-04-20. Retrieved 2021-04-20.
^ Helmenstine, Anne Marie (2020). "Le Chatelier's Principle Definition". ThoughtCo. Archived from the original on 2021-04-20. Retrieved 2022-03-09.
^ Münster, A. (1970), pp. 173–176.
^ Bailyn, M. (1994), pp. 312–318.
^ Bailyn, M. (1994), p. 313.
^ Kay, J. J. (February 2000) [1999]. "Application of the Second Law of Thermodynamics and Le Chatelier's Principle to the Developing Ecosystem". In Muller, F. (ed.). Handbook of Ecosystem Theories and Management. Environmental & Ecological (Math) Modeling. CRC Press. ISBN 978-1-56670-253-9. As systems are moved away from equilibrium, they will utilize all available avenues to counter the applied gradients... Le Chatelier's principle is an example of this equilibrium seeking principle. For full details, see: Ecosystems as Self-organizing Holarchic Open Systems: Narratives and the Second Law of Thermodynamics, 2000, p. 5, CiteSeerX 10.1.1.11.856
^ a b Atkins (2017) et.al., p. 192 harvnb error: no target: CITEREFAtkins_(2017)_et.al. (help).
^ Callen, H.B. (1960/1985), Chapter 8, pp. 203–214.
^ Bailyn, M. (1994), Chapter 8, Part A, pp. 312–319.
^ Prigogine, I., Defay, R. (1950/1954), pp. 268–269.
^ Prigogine, I., Defay, R. (1950/1954), p. 265.
^ a b Gall, John (2002). The Systems Bible (3rd ed.). General Systemantics Press. The System always kicks back
^ "The Biophysical Basis for the Graphical Representations". Archived from the original on 2009-01-23. Retrieved 2009-05-04.
^ Samuelson, Paul A. (1983).
^ Silberberg, Eugene (1971). "The Le Chatelier Principle as a Corollary to a Generalized Envelope Theorem". Journal of Economic Theory. 3 (2): 146–155. doi:10.1016/0022-0531(71)90012-3.
Bibliography of cited sources[edit]
Atkins, P.W. (1993). The Elements of Physical Chemistry (3rd ed.). Oxford University Press.
Bailyn, M. (1994). A Survey of Thermodynamics, American Institute of Physics Press, New York, ISBN 0-88318-797-3.
Callen, H.B. (1960/1985). Thermodynamics and an Introduction to Thermostatistics, (1st edition 1960) 2nd edition 1985, Wiley, New York, ISBN 0-471-86256-8.
Münster, A. (1970), Classical Thermodynamics, translated by E.S. Halberstadt, Wiley–Interscience, London, ISBN 0-471-62430-6.
Prigogine, I., Defay, R. (1950/1954). Chemical Thermodynamics, translated by D.H. Everett, Longmans, Green & Co, London.
Samuelson, Paul A (1983). Foundations of Economic Analysis. Harvard University Press. ISBN 0-674-31301-1.
YouTube video of Le Chatelier's principle and pressure
Retrieved from "https://en.wikipedia.org/w/index.php?title=Le_Chatelier%27s_principle&oldid=1136507394"
Equilibrium chemistry
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redpajama_set_name: RedPajamaGithub


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Jennifer Zambone
Jennifer Zambone is the Publications Manager at the Mercatus Center at George Mason University.[1] Prior to this she worked as the Washington D.C.-based director of Africa Fighting Malaria, a pro-DDT lobby group.
A biographical note from 2001 on the website of the Competitive Enterprise Institute stated that she "studies environmental health risks and air policy. Her recent work has focused on science and public health, pesticides, arthropod borne disease, and toxic air pollutants."[2]
1 Africa Fighting Malaria
2 Positions held
3.3.1 Articles by Zambone
Africa Fighting Malaria
Zambone was the Director of Africa Fighting Malaria between 2003 and 2005. (In 2003 Zambone, who was the group's only paid employee, earned $35,000.[3] The following year Zambone's renumeration for her 40 hours a week had jumped from $35,00 to $60,000).[4] In 2005 Zambone's remuneration dropped back down to $35,000.[5]
Competitive Enterprise Institute, Environmental Policy Analyst 2001
Africa Fighting Malaria, 2003-2005
Mercatus Center at George Mason University, Associate Director of the Regulatory Studies Program
↑ "Jennifer Zambone: Publications Manager", Mercatus Center, accessed January 2009.
↑ "Jennifer Zambone: Environmental Policy Analyst", Competitive Enterprise Institute, accessed January 2004.
↑ Africa Fighting Malaria, "Africa Fighting Malaria Annual Report", January 2003, page 4.
↑ Africa Fighting Malaria, "Africa Fighting Malaria Annual Report 2004", August 2005, pages 1 and 4.
Articles by Zambone
Jennifer Zambone, "Managing Malaria", National Review Online, April 6, 2004.
Jennifer Zambone, "A Martha Is a Terrible Thing to Waste", TCS Daily , August 3, 2004.
Jennifer Zambone, "Malaria in the USA", undated, accessed Jan 2009.
Roger Bate, Richard Tren, Jasson Urbach, Jennifer Zambone, "Considerations for the Use of DDT in Malaria Control", Health Policy and Development, October 2004.
Jennifer Zambone, "Vaccine Vacancy", National Review Online, October 15, 2004.
Jennifer Zambone, "Punting Globally", TCS Daily, April 25, 2005.
Retrieved from "https://www.sourcewatch.org/index.php?title=Jennifer_Zambone&oldid=394734"
Think tanks/personnel

redpajama_set_name: RedPajamaCommonCrawl


text:
Gran Turismo 5 3D Review: Hands-on first impressions
GT5 finally lands in the UK in all its 3D glory
By Luke Johnson 2010-10-21T23:00:00.293Z
Gran Turismo 5 Gamer Setup
T3 get behind the wheel of Gran Turismo
Gran Turismo 5, the most anticipated and surely most delayed title in gaming history has finally touched down in the UK.
The T3 VIP Reader Event at Selfridges' London Oxford Street store saw the racing sim on its first ever free consumer outing.
-Check out these Gran Turismo 5 (GT5) 3D pics
Having cost a reported $60 million to create and with a delay of more than five years for the title to arrive, the question on the lips of everyone with an interest in the definitive racing title is "Is it really worth the wait?"
- Gran Turismo 5 in action photographs: Click here
With half an hour before the lucky VIP readers arrived, T3 took to the driving seat of the ultimate Gran Turismo 5 3D racing setup - bucket seat, Logitech Driving Force GT Wheel plus Pedals and a HD Sony 3D TV - to bring you our first impressions of Gran Turismo 5 (GT5).
3D is understandably one of the key talking points in the games industry at present, with Gran Turismo 5 lined up to be the biggest title release in the new format to date.
First impressions of GT5's 3D quality are somewhat underwhelming. Donning a pair of active shutter specs one might expect to be immersed into a world of near misses and stunningly deep backdrops, but the use of 3D seems to in fact take away some of the edge of what is otherwise graphical supremacy.
The extra dimensional tech comes in to its own as you continue with the game. When racing at close quarters with other vehicles and as racers bunch up in slow corners, the obsession to detail and enormous levels of precision insisted on by the game's creators combine with the 3D experience to take on a truly stunning aspect - well worth the 3D sticker price.
Graphically little more can be said about Gran Turismo 5 than simply, wow. Surpassing all the franchises previous releases and most other games on the market, the level of detail seen in the vehicles and environments alike is nothing short of astounding.
Tracks such as the Top Gear Test Track are replicated in the game in inch-perfect detail with backdrops replicating those of real life. While the cars themselves are perfectly true to life, a brief dabble with the in car camera failed to impress as much as other aspects of the game.
The level of realism found in GT5 is not limited to its graphical superiority, its physics are also far beyond anything seen in previous titles. Braking too hard into a corner or tapping the accelerator at the microsecond and you will quickly find yourself fighting against a few hundred horses pushing and pulling the car in all the directions you are trying not to go.
In terms of steering, cars in the game appear to respond to their true to life counterparts with vehicles notorious for poor handling being loose in the corners and forcing you to fight against vicious under and over steer. The meticulous nature with which this game has been constructed can at times be infuriating when a strong lap is ruinied by a minor lapse in concentration. This frustration is soon forgotten, however, as you cross the line for the next lap and once again submit to the true brilliance of this long awaited title.
Were you at the T3 VIP reader night? Share you thoughts of Gran Turismo 5 in 3D with us via the T3 Twitter and Facebook accounts.
More about Gran Turismo
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A new trailer has been posted online showing the new visual style and cars
By T3 Online • 2013-05-18T20:01:00.137Z
Last chance! Best Amazon Prime Day Nerf deals and paddling pools: save up to £20!
Nerf foam blasters and laser playsets all get money off, as well as some extremely cool dinosaur paddling pools
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Lego Star Wars, Lego Harry Potter and Sylvanian Families animals and building get big discounts… that end soon
Sony customer survey hints at Gran Turismo PS Vita release
Forget Gran Turismo 6 landing for the Sony PS4, GT for PS Vita is reportedly in the works
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text:
Shortbread (von engl. short dough "Mürbeteig", also etwa "mürbes Brot") ist ein schottisches süßes Mürbeteiggebäck. Das klassische Rezept besteht aus einem Teil Zucker, zwei Teilen Butter und drei Teilen Mehl (Gewichtsteile).

Shortbread wird üblicherweise in drei verschiedenen Formen gebacken: Die verbreitetste Form sind die quaderförmigen, fingerlangen "Shortbread Fingers". Die anderen sind knapp einen Zentimeter dicke "Shortbread Rounds" von rund fünf Zentimetern Durchmesser. Bei einer anderen Form werden aus Scheiben von etwa 15 bis 20 Zentimetern Durchmesser vorgestanzte Kreissegmente, so genannte "Petticoat Tails", herausgebrochen.

Im Vereinigten Königreich, besonders in Schottland, gehört Shortbread zu den beliebtesten Gebäckarten, die besonders gerne zur klassischen "Tea Time" gereicht werden.

Literatur

Weblinks

Feine Backware
Schottische Küche

redpajama_set_name: RedPajamaWikipedia


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Q: Alguien sabe como puedo resolver esto La funcion recibe un objeto "persona".
// de la forma:
// {
//  nombre: 'Lionel
//  apellido: 'Messi',
//  invitado: true
//  }
// Si tiene la propiedad "invitado" y, además, tiene las propiedades "nombre" y "apellido", tomar esos valores y retorna:
// "Lionel Messi, un gusto tenerlo nuevamente! Bienvenido".
// Si tiene la propiedad "invitado" y solo tiene la propiedad "apellido", retornar:
// "Bienvenido Sr. Messi".
// Si tiene la propiedad "invitado" y solo tiene la propiedad "nombre", retornar:
// "Hola Lionel, tu mesa está lista".
// En caso de que no tenga la propiedad "invitado" retornar:
// "Disculpe señor, no está invitado a la fiesta".
// Micódigo hasta este momento:

    const cliente = {
    nombre: "nombre",
    apellido: "apellido",
    invitado: true,
    saludo1: function() {
        return this.nombre + " " + this.apellido + " un gusto tenerlo nuevamente! Bienvenido";
        },
    saludo2: function(){
        return "Bienvenido Sr." + this.apellido;
        },
    saludo3: function(){
        return "Hola " + this.nombre + ", tu mesa está lista";
        },
    sinSaludo: function(){
       return "Disculpe Señor, no está invitado a la fiesta";
        }

}

A: Esto lo resuleves con condicionales. En lugar de 4 métodos usa uno solo: saludo que devolverá el valor adecuado según el contenido del objeto. Doy por supuesto que los datos de nombre y apellido serán strings vacios si no se asigna algún valor.
Uso trim por si nombre o apellido son cadenas de espacios. Considero que no tener la propiedad invitado significa invitado:false. Y no tener nombre o apellidos significa que son cadenas vacías.

const cliente = {
    nombre: "",
    apellido: "",
    invitado: true,
    saludo: function() {
    saludo='';
    //comprobamos que hay nombre y/o apellido
    if( this.nombre.trim()+this.apellido.trim()!='')
      {
      //comprobamos que está invitado
      if(this.invitado){
          if(this.nombre.trim() !='' && this.apellido.trim() !='')
              saludo = this.nombre + " " + this.apellido + " un gusto tenerlo nuevamente! Bienvenido";
          else if (this.nombre.trim() =='' &&  this.apellido.trim() !='')
              saludo= "Bienvenido Sr." + this.apellido;
          else if (this.nombre.trim() !='' &&  this.apellido.trim() =='')
              saludo = "Hola " + this.nombre + ", tu mesa está lista";
      }
    else {
          saludo= "Disculpe Señor, no está invitado a la fiesta";
        }
      }
   return saludo;
   }
}
console.log(cliente.saludo())

A: La forma en la que escribí esta en JS ES6, podrías buscar información sobre todo eso ya que te ayuda mucho a como escribir tu código.
Para obtener la solución a tu problema se hace mediante condicionales, preguntando una y otra vez si cumple ciertos requisitos para entrar o no, y así generar una respuesta.
La destructuración se utiliza para obtener de manera mas efectiva los atributos de un objeto, y no estar escribiendo objeto.atributo
En tu enunciado indicaste que tienes que crear una funcion que reciba un objeto por lo tanto el objeto y la funcion deben estar separados, y el objeto lo puedes destructurar en la misma linea que lo recibe: saludo = (cliente) => { ... o saludo = ({ nombre, apellido, invitado }) => { ...
const nuevoCliente = {
  nombre: '',
  apellido: '',
  invitado: true,
}

const saludo = (cliente) => { // Funcion flecha
  const { nombre, apellido, invitado } = cliente; // Destructuracion

  let respuesta = '';

  if (invitado) {
    if (nombre && apellido) {
      respuesta = `${nombre} ${apellido} un gusto tenerlo nuevamente`
    } else if (nombre) {
        respuesta = `Hola ${nombre} tu mesa esta lista`
    } else if (apellido) {
      respuesta = `Bienvenid@  Sr/a ${apellido}`
    } else {
      respuesta = `El empleado debe tener un nombre o un apellido`
    }
  } else {
    respuesta = 'Usted no esta invitado';
  }

  return respuesta;
}

saludo(nuevoCliente)

Te aconsejo encarecidamente que busques información sobre las nuevas formas de escribir código en JavaScript, eso te ayudara bastante.
Espero haberte ayudado!

redpajama_set_name: RedPajamaStackExchange


text:
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Home » Celebrities » Vanessa Kirby on Assault Allegations Against Shia LaBeouf: I Stand With Abuse Victims
Vanessa Kirby on Assault Allegations Against Shia LaBeouf: I Stand With Abuse Victims
'The Crown' alum finally breaks her silence after her 'Pieces of a Woman' co-star was sued by his former girlfriend FKA twigs over alleged assault and sexual battery during their relationship.
AceShowbiz –Vanessa Kirby has finally broken her silence on Shia LaBeouf's abuse allegations. A few weeks after her "Pieces of a Woman" co-star was sued by his ex-girlfriend FKA twigs for alleged assault and sexual battery during their relationship, the Martha Weiss depicter stressed that she does "stand with abuse victims."
The actress known for her portrayal of Princess Margaret on "The Crown" shared her two cents on the matter in a new interview with The Sunday Times. "I stand with all survivors of abuse and respect the courage of anyone who speaks their truth," she stated. "Regarding the recent news, I can't comment on an ongoing legal case."
While Kirby did not directly condemn LaBeouf with her statement, Netflix made a harsher response to the assault allegations. The streaming service removed the actor from the For Your Consideration page of "Pieces of a Woman", which features the movie's synopsis and stills, and from any award consideration.
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LaBeouf's former girlfriend twigs took him to court back on December 11, 2020. The musician, whose real name is Tahliah Barnett, filed the lawsuit in Los Angeles as she accused the "Transformers" actor of physical abuse, sexual battery and infliction of emotional distress during their months-long relationship since late 2018.
LaBeouf has since responded to the accusations by offering an apology. "I'm not in any position to tell anyone how my behavior made them feel," he said. "I have no excuses for my alcoholism or aggression, only rationalizations. I have been abusive to myself and everyone around me for years. I have a history of hurting the people closest to me. I'm ashamed of that history and am sorry to those I hurt. There is nothing else I can really say."
While LaBeouf expressed his remorse for his aggressive behavior, he claimed that "many of these allegations are not true." Though so, he was said to have sought for a "long-term inpatient treatment" following the scandal. "[He] needs help and he knows that," his lawyer Shawn Holley told Variety. "We are actively seeking the kind of meaningful, intensive, long-term inpatient treatment that he desperately needs."
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text:
Events in the year 1868 in Spain.

Incumbents
Monarch - Isabella II until September 30

Events
September 19–27 - Glorious Revolution (Spain)

Births

Deaths
April 23 - Ramón María Narváez, 1st Duke of Valencia

1860s in Spain


text:
Aski Shahr (, also Romanized as Askī Shahr; also known as Ask Shahr) is a village in Balghelu Rural District, in the Central District of Ardabil County, Ardabil Province, Iran. At the 2006 census, its population was 70, in 15 families.

References

Towns and villages in Ardabil County


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