CHEMISTRY HELP PLEASE!!?
Title: Chemistry Help Needed
Body:
I am studying the decomposition of a metal oxide into its elements, represented by the following reaction:
M2O (s) → 2M (s) + 1/2 O2 (g)
The standard Gibbs energy changes for the substances involved are as follows:
- ΔG for M2O: -6.30 kJ/mol
- ΔG for M: 0 kJ/mol
- ΔG for O2: 0 kJ/mol
I have a few questions regarding this reaction:
1) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? 2) What is the equilibrium constant for this reaction, as written, in the forward direction at 298 K? 3) What is the equilibrium pressure of O2 over M (s) at 298 K?
Thank you for your assistance!
2 Answers
1) Delta G = 0 - (-6.3) = 6.3
2) delta G = -RTln(K)
6.3 = -R298ln(K)
ln(K) = -2.54*10^-3
K = 1 (maybe delta G = 6.3 kJ)
3)
K = 1 = p^0.5
p = 1
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