Free Energy of Reaction -- Temperature Dependence?

2NH3(g) + 3O2(g) + 2CH4(g)

1000°C
-------->
Pt - Rh

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.)


a. Calculate ΔH° for this equation.

b. Calculate ΔS° for this equation.

c. Calculate ΔG° at 161°C, for this equation.

Answer:
I'm not looking up the values for you. You can calculate those DH and DS values by adding up the values using the stoichimetric coefficients as factors for each. Remember: "Products minus reactants."

Then you use DG = DH - TDS to calculate DG.

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