<br>Above reaction is endothermic and hence the actual temperature of the reaction vessel (isolated — Thermodynamics and Thermochemistry Chemistry Question
Question
$2\text{MnO}_4^- + 16\text{H}^+ + 10\text{Cl}^- \to 2\text{Mn}^{2+} + 5\text{Cl}_2\text{(g)} + 8\text{H}_2\text{O}$<br>Above reaction is endothermic and hence the actual temperature of the reaction vessel (isolated from the surrounding) may be different from that expected. Given that the initial temperature of the reaction vessel was used in the calculations, how would, this affect the predicted value of moles of $\text{Cl}_2$ ($n$), according to equation: $n = PV/RT$
💡 Solution & Explanation
Since the reaction is endothermic and the vessel is isolated, the actual temperature ($T_{\text{actual}}$) drops below the initial expected temperature ($T_{\text{initial}}$). Because $n \propto 1/T$, using the higher $T_{\text{initial}}$ in the calculation results in a predicted $n$ that is less than the actual $n$.