Question

For the reaction: $2H_{2}O(l) \rightleftharpoons 2H_{2}(g)+O_{2}(g)$ at 25°C, the equilibrium constant is 7.0 × $10^{-84}$.
(i) Calculate the standard Gibbs energy formations of water at 25°C.
(ii) ΔH°($H_{2}O$) = – 280 kJ $mol^{-1}$. Calculate the entropy change for the reaction.

Answer 1

Answer:

ii) ΔH°($H_{2}O$) = – 280 kJ $mol^{-1}$. Calculate the entropy change for the reaction.

Explanation:

For the reaction: $2H_{2}O(l) \rightleftharpoons 2H_{2}(g)+O_{2}(g)$ at 25°C, the equilibrium constant is 7.0 × $10^{-84}$.