Consider the reaction: CH3OH(g) → CO(g) + 2 H2(g). Calculate ΔG for this reaction at 25 °C under the following conditions: i. PCH3OH = 0.855 atm ii. PCO = 0.125 atm iii. PH2 = 0.183 atm.

Verified step by step guidance

1. <insert step 1> Identify the reaction: CH3OH(g) → CO(g) + 2 H2(g). This is a decomposition reaction where methanol decomposes into carbon monoxide and hydrogen gas.
2. <insert step 2> Use the equation for Gibbs free energy change under non-standard conditions: $\mathrm{\Delta }G=\mathrm{\Delta }{G}^{\circ }+RT\ln Q$, where $R$ is the gas constant (8.314 J/mol·K), $T$ is the temperature in Kelvin, and $Q$ is the reaction quotient.
3. <insert step 3> Convert the temperature from Celsius to Kelvin: $T=25+273.15=298.15\text{ K}$.
4. <insert step 4> Calculate the reaction quotient $Q$ using the partial pressures: $Q=\frac{P_{CO}\cdot (P_{H_2}{)}^2}{P_{C{H}_{3}OH}}=\frac{0.125\cdot (0.183{)}^2}{0.855}$.
5. <insert step 5> Substitute the values into the Gibbs free energy equation: $\mathrm{\Delta }G=\mathrm{\Delta }{G}^{\circ }+(8.314\times 298.15)\ln Q$. Note that $\mathrm{\Delta }{G}^{\circ }$ (standard Gibbs free energy change) needs to be provided or looked up in a table of standard values.