Water becomes cold on mixing energy drink I noticed that the temperature of water decreases noticeably when I mix an energy drink (Glucon-D) in it. The ingredients mentioned on the pack are majorly glucose (52%) and sucrose (45%). I believe that this is due to the inversion of sucrose being an endothermic reaction
$$\ce{C12H22O11 + H2O + \Delta -&gt; \underset{glucose}{C6H12O6} + \underset{fructose}{C6H12O6}}$$
However, I could not find any sources on the internet to validate this. Please confirm/disprove this hypothesis and also explain the correct reason for this.

EDIT: After everyone's recommendations of sticking a thermometer in my drink, I did so and came up with the following observations:
\begin{array}{|c|c|c c|c|}
\hline
m_\text{drink} &amp; V_\ce{H2O} &amp; T_i &amp; T_f &amp; \Delta T\\
\hline
\pu{14.85 g} &amp; \pu{200 ml} &amp; \pu{20.3°C} &amp; \pu{19.5 °C} &amp; \pu{0.7 °C}\\
\hline
\end{array}

Some elementary thermochemistry gives me the result that $\Delta H_\text{solution}$ for the energy drink is $\approx \pu{39.6 J g-1}$.
Well, the solution enthalpy of sugars is positive.
I found these numbers on the internet


$\ce{C12H22O11}$ (sugar(sucrose)) : 5.4 kJ/mol
$\ce{C6H12O6}$ (glucose) : 11 kJ/mol
$\ce{C6H12O6·H2O}$ (glucose monohydrate) : 19 kJ/mol


So if your "energy drink" is a dry powder (and not a readymade drink in an aluminum can), this could explain your observation.

You should however put a thermometer into your experiment, and get us some numbers. As is, my above is just another piece of guesswork.