(a) Determine Δr H^∘ for the reaction: CO(g)+(1)/(2) O2(g) →CO2(g) given that, at 298 K Δf H^∘(C

step 1 Thermodynamics is the branch of physics that deals with the relationships between heat and other

(a) Determine Δr H^∘ for the reaction: CO(g)+(1)/(2) O2(g)...

(a) Determine $\Delta_{\mathrm{r}} H^{\circ}$ for the reaction: $\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})$ given that, at $298 \mathrm{K}$ $\Delta_{\mathrm{f}} H^{\circ}(\mathrm{CO}, \mathrm{g})=-110.5 \mathrm{kJ} \mathrm{mol}^{-1}$ and $\Delta_{\mathrm{f}} H^{\mathrm{o}}\left(\mathrm{CO}_{2}, \mathrm{g}\right)=-393.5 \mathrm{kJ} \mathrm{mol}^{-1}$ (b) Calculate $\Delta_{\mathrm{r}} H^{\circ}(320 \mathrm{K})$ for the above reaction given that $C_{P}(298-320 \mathrm{K})$ for $\mathrm{CO}(\mathrm{g}), \mathrm{O}_{2}(\mathrm{g})$ and $\mathrm{CO}_{2}(\mathrm{g})=29.2,29.4$ and $37.2 \mathrm{JK}^{-1} \mathrm{mol}^{-1}$ respectively.

(a) Determine $\Delta_{\mathrm{r}} H^{\circ}$ for the reaction:
$\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})$
given that, at $298 \mathrm{K}$ $\Delta_{\mathrm{f}} H^{\circ}(\mathrm{CO}, \mathrm{g})=-110.5 \mathrm{kJ} \mathrm{mol}^{-1}$ and
$\Delta_{\mathrm{f}} H^{\mathrm{o}}\left(\mathrm{CO}_{2}, \mathrm{g}\right)=-393.5 \mathrm{kJ} \mathrm{mol}^{-1}$
(b) Calculate $\Delta_{\mathrm{r}} H^{\circ}(320 \mathrm{K})$ for the above reaction
given that $C_{P}(298-320 \mathrm{K})$ for $\mathrm{CO}(\mathrm{g}), \mathrm{O}_{2}(\mathrm{g})$ and
$\mathrm{CO}_{2}(\mathrm{g})=29.2,29.4$ and $37.2 \mathrm{JK}^{-1} \mathrm{mol}^{-1}$
respectively.

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Key Concepts

Kirchhoff's Law

Kirchhoff's Law in thermochemistry explains how the enthalpy change of a reaction varies with temperature. It states that the change in the reaction enthalpy when the temperature is altered can be calculated by integrating the difference in heat capacities between the products and reactants over the desired temperature range. This provides a means to correct the reaction enthalpy from one temperature to another.

Heat Capacity in Thermochemistry

Heat capacity, particularly at constant pressure (Cp), is a measure of the amount of heat required to raise the temperature of a mole of substance by one Kelvin. In the context of reaction enthalpy calculations, it is used to determine how much the enthalpy of a system changes with temperature, thus allowing for adjustments in the enthalpy when the temperature deviates from standard conditions.

Standard Reaction Enthalpy

This concept involves calculating the overall enthalpy change of a chemical reaction by using the standard enthalpies of formation of the reactants and products. By applying Hess's Law, one determines the reaction enthalpy using the formula ?rH° = ?(n×?fH° of products) ? ?(n×?fH° of reactants). This approach allows for the determination of heat exchange under standard conditions, even if the reaction cannot be measured directly.

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