How to Determine the Rate Law knowing time and concentrations Consider the hypothetical reaction described by the following equation:

$$\ce{3 A + 2 B -&gt; C}$$

Reagent B was added in excess and the following time concentration data was obtained.

\begin{array}{cr}
A\ [\mathrm{10^{-3}\ mol\cdot L^{-1}}] &amp; \mathrm{time [s]} \\ \hline
5.0 &amp; 10\\
2.9 &amp; 50\\
1.9 &amp; 80\\
1.1 &amp; 120\\
0.7 &amp; 150\\
\end{array}

(i) Derive the relevant integrated rate law and hence find the rate constant. 

I am thinking that to solve this question you just sub the values into the integrate rate laws and see if it produces a linear relationship. 

Is this correct? Also could you please suggest a faster method of solving this type of question.

Thank you.
You could plot the data to determine the order of the reaction.  I would use Microsoft Excel to do this.  Reproduce the data and then add columns that calculate the $\ln [A]$ and $\frac{1}{[A]}$.  Then plot $[A]$, $\ln [A]$ ,and $\frac{1}{[A]}$ vs. time (I would use separate plots).  The plot that gives the "best" linear fit (which you can assess using the $R^2$ value), corresponds to the appropriate integrated rate law.  


If $[A]$ vs. time is linear, then the reaction is zero order.
If $\ln [A]$ vs. time is linear, then the reaction is first order.
If $\frac{1}{[A]}$ vs. time is linear, then the reaction is second
order.


Hope this helps.