For CO(g)+ H₂(g)→ H₂CO(g),Δ_rH° = -5.36 kJ/mol,and Δ_rS° = -109.8 J/mol K.What is the temperature at which K_eq is 1.0 × 10^-2? A)5.19 × 10³ °C B)218 °C C)25 °C D)-198 °C E)-237 °C

Question

Quizplus · Accepted Answer

The equation for Gibbs free energy change is:

ΔG1U1B1 = ΔH1U1B1 - TΔS1U1B1

At equilibrium, ΔG1U1B1 = 0, so we can rearrange the equation:

T = ΔH1U1B1/ΔS1U1B1

Substituting the values given in the question, we get:

T = (-5.36 kJ/mol) / (-109.8 J/mol K) = 48.86 K = -224.29 °C

However, the temperature is given in degrees Celsius, so we need to convert it:

T = -224.29 °C + 273.15 = -198.14 °C

Therefore, the answer is D.

For CO(g)+ H2(g)→ H2CO(g),ΔrH° = -5

For CO(g)+ H₂(g)→ H₂CO(g),Δ_rH° = -5