Question

2 H2S (g) + SO2 (g) <===> ƒnƒn3 S (s) + 2 H2O (g)
1) At 298 K, the standard enthalpy change, H¢X, for the reaction represented below is -145 kilojoules.
(a) Predict the sign of the standard entropy change, S¢X, for the reaction. Explain the basis foryour prediction.

(b) At 298 K, the forward reaction (i.e., toward the right) is spontaneous. What change, if any, would occur in the value of G¢X for this reaction as the temperature is increased? Explain your reasoning using thermodynamic principles.

(c) What change, if any, would occur in the value of the equilibrium constant, Keq, for the situation described in (b)? Explain your reasoning.

(d) The absolute temperature at which the forward reaction becomes non spontaneous can be predicted. Write the equation that is used to make the prediction. Why does this equation predictonly an approximate value for the temperature?

Answer 1

a) because the moles of gas decreases, there is less disorder and the delta s value is negative.
b) the delta g value would become less negative and eventually positive with enough heat.
c) the keq would become lower.
d) (delta g)= (delta h) - T(delta s)
the delta g value would be replaced with 0.