Free Energy of Reaction -- Temperature Dependence True or False?
1000°C
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Pt - Rh
2HCN(g) + 6H2O(g)
a. The equilibrium position for this reaction is further to the right at lower temperatures.
b. Thermodynamically, this reaction is spontaneous only below a certain temperature.
c. This reaction is endothermic at room temperature.
d. At temperatures significantly lower than 1000°C this reaction is not spontaneous.
e. The high temperature required for this process is needed for kinetic reasons.
Answer:
Higher temperature favors the more disordered side of the reaction (higher entropy). You can deduce this readily from the Gibbs Helmholtz equation.
More particles of gas means more entropy.
Seven particles of gas on the left, 8 on the right.
Thus higher temperature will favor the products more.
To get quantitative information or to decide endo or exothermicity we need the enthalpies of formation of the products and reactants. You provide those. I'm not looking them up.
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