For the reaction 2CO(g) + 2NO(g) ? 2CO2(g) + N2(g) ?H° = -746.6 kJ and ?S° = -198.0 J/K The maximum amount of work that could be done when 1.96 moles of CO(g) react at 325 K, 1 atm is [ ] kJ. Assume that ?H° and ?S° are independent of temperature.
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Tianyu L.
Consider the reaction: $4 \mathrm{CO}(g)+2 \mathrm{NO}_{2}(g) \longrightarrow 4 \mathrm{CO}_{2}(g)$ $+\mathrm{N}_{2}(g) .$ Using the following information, determine $\Delta H^{\circ}$ for the reaction at $25^{\circ} \mathrm{C} .$ $$ \begin{array}{ll}{\mathrm{NO}(g)} & {\Delta H^{\circ}=+91.3 \mathrm{kJ} / \mathrm{mol}} \\ {\mathrm{CO}_{2}(g)} & {\Delta H^{\circ}=-393.5 \mathrm{kJ} / \mathrm{mol}} \\ {2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g)} & {\Delta H^{\circ}=-116.2 \mathrm{kJ}} \\ {2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)} & {\Delta H^{\circ}=-566.0 \mathrm{kJ}}\end{array} $$
For the reaction 2Fe(s) + 3Cl2(g) → 2FeCl3(s) ΔG° = -673.1 kJ and ΔS° = -440.3 J/K at 286 K and 1 atm. The maximum amount of work that could be done by this reaction when 1.70 moles of Fe(s) react at standard conditions at this temperature is ____ kJ.
Madhur L.
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