Calculate the pressure of O2 (in atm) over a sample of NiO at 25.00°C if ΔG o = 212 kJ/mol for the reaction. For this calculatio

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Bezzdna

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Calculate the pressure of O2 (in atm) over a sample of NiO at 25.00°C if ΔG o = 212 kJ/mol for the reaction. For this calculatio

n, use the value R = 8.3144 J/K·mol. NiO(s) ⇌ Ni(s) + 1 2 O2(g)

Chemistry

1 answer:

Anarel [2.7K] · Answer 1 · 2026-03-06T10:55:13+03:00

Based on the given information:
Δ G° = 212 KJ/mol, the temperature is calculated as 25+273 = 298 K, and the gas constant R equals 0.008314 KJ/mol.

The reaction can be characterized as NiO(s) ⇌ Ni(s) + $\frac{1}{2} O_{2 _{(g)}$ . To determine the oxygen pressure, we can apply Gibb's free energy equation with the quotient remaining, which is expressed as: ΔG = ΔG° +RT lnQ. At equilibrium, Q equals K, leading ΔG to be 0;
therefore, it simplifies to 0 = ΔG° + RT ln K. By rearranging, we arrive at ln K = ΔG° / (RT). Calculating gives, ln K = 212 / (0.00831 X 298) = 85.6.
Thus, we find K = 1.51 X $10^{37}$ .
Consequently, with K = 1.51 X $10^{37}$ ,

Ultimately, K = $(PO_{2})^ \frac{1}{2}$ . Therefore, (1.51 X $10^{37}$ ) $^ \frac{1}{2}$ results in 3.87 X $10^{18}$ .
The resulting pressure of oxygen will be = 3.87 X $10^{18}$ Pa.

To convert Pa to atm, we find 3.756 X $10^{13}$ atm.