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: \( \Delta G = \Delta G^\circ + RT \ln Q \), 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: \( Q = \frac{P_{CO} \cdot (P_{H_2})^2}{P_{CH_3OH}} = \frac{0.125 \cdot (0.183)^2}{0.855} \).
5. <insert step 5> Substitute the values into the Gibbs free energy equation: \( \Delta G = \Delta G^\circ + (8.314 \times 298.15) \ln Q \). Note that \( \Delta G^\circ \) (standard Gibbs free energy change) needs to be provided or looked up in a table of standard values.