Free Energy of Reaction -- Temperature Dependence
2NH3(g) + 3O2(g) + 2CH4(g) 2HCN(g) + 6H2O(g)
The above reaction is used in the industrial production of hydrogen cyanide. Consider the relevant thermodynamic data from the appendices of your text. (The tabulated values ΔH°f and S° are for 25°C. For the purposes of this question assume that ΔH° and ΔS° are invariant with temperature. This is not actually true but would generally be a reasonable approximation over "small" temperature ranges.)
Calculate ΔH° for this equation.
1 pts
Tries 0/8
Calculate ΔS° for this equation.
1 pts
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Calculate ΔG° at 882°C, for this equation.
1 pts
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Are the following statements about this process True or False?
True False At temperatures significantly lower than 1000°C this reaction is not spontaneous.
True False The high temperature required for this process is needed for kinetic reasons.
True False The equilibrium position for this reaction is further to the left at lower temperatures.
True False Thermodynamically, this reaction is spontaneous only above a certain temperature.
True False This reaction is endothermic at room temperature.