Consider the decomposition of a metal oxide into its elements, where M represents a generic metal. The reaction can be represented as follows: [ \text{M}_2\text{O (s)} \rightarrow 2\text{M (s)} + \frac{1}{2}\text{O}_2 \text{ (g)} ] The standard Gibbs energy values for the substances involved are: (\Delta G_{\text{M}_2\text{O}} = -6.30 \, \text{kJ/mol}) (\Delta G_{\text{M}} = 0 \, \text{kJ/mol}) (\Delta G_{\text{O}_2} = 0 \, \text{kJ/mol}) 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 (\text{O}_2) over (\text{M (s)}) at 298 K?

Oct 30, 2024

Consider the decomposition of a metal oxide to its elements

Consider the decomposition of a metal oxide into its elements, where M represents a generic metal. The reaction can be represented as follows:

[ \text{M}_2\text{O (s)} \rightarrow 2\text{M (s)} + \frac{1}{2}\text{O}_2 \text{ (g)} ]

The standard Gibbs energy values for the substances involved are:

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 (\text{O}_2) over (\text{M (s)}) at 298 K?

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Jan 21, 2025

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)

K = 1 = p^0.5

p = 1

Feb 01, 2025

K is 0.0786

p is 0.00619

but his way is correct

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