This question is about chemical equilibrium and thermodynamics.
Carbon monoxide, CO\text{CO}CO, and hydrogen, H2\text{H}_2H2, react to form methanol, CH3OH\text{CH}_3\text{OH}CH3OH, in the reversible reaction shown below:
CO(g)+2H2(g)⇌CH3OH(g)ΔH=−92.0 kJ mol−1, ΔS=−215 J mol−1 K−1 \text{CO}(\text{g}) + 2\text{H}_2(\text{g}) \rightleftharpoons \text{CH}_3\text{OH}(\text{g}) \quad \Delta H = -92.0\text{ kJ mol}^{-1}, \; \Delta S = -215\text{ J mol}^{-1}\text{ K}^{-1} CO(g)+2H2(g)⇌CH3OH(g)ΔH=−92.0 kJ mol−1,ΔS=−215 J mol−1 K−1A dynamic equilibrium exists in a closed system. State one other feature of a dynamic equilibrium.
Show that the formation of CH3OH\text{CH}_3\text{OH}CH3OH is feasible at 25∘C25^\circ\text{C}25∘C.
Determine the maximum temperature, in K\text{K}K, for feasibility. Give your answer to an appropriate number of significant figures.
A chemical engineer mixes together 1.50 mol of CO(g)\text{CO}(\text{g})CO(g) and 2.50 mol of H2(g)\text{H}_2(\text{g})H2(g) in a sealed reactor, and the mixture is allowed to reach equilibrium. At equilibrium, 60% of the CO(g)\text{CO}(\text{g})CO(g) has been converted to CH3OH(g)\text{CH}_3\text{OH}(\text{g})CH3OH(g), and the total pressure is 2.00 MPa.
Calculate KpK_pKp, in MPa−2\text{MPa}^{-2}MPa−2, for this reaction. Give your answer to 3 significant figures.
The engineer then repeats the experiment three times. In each experiment, the engineer makes one change but uses the same initial amounts of CO\text{CO}CO and H2\text{H}_2H2.
Complete the table to show the predicted effect of each change compared with the original experiment. Only use the words greater, smaller, or same.
| Change | KpK_pKp | Equilibrium amount of CH3OH(g)\text{CH}_3\text{OH}(\text{g})CH3OH(g) | Initial rate |
|---|---|---|---|
| Temperature increase | |||
| Pressure increase | |||
| Catalyst added |
