Which of the following phase‐transition processes cannot be applied using the Clausius–Clapeyron equation?

For an ideal gas, which relation is correct? 

When the reaction quotient Q is greater than the equilibrium constant K, the reaction will: 

The maximum work that can be delivered to the surroundings is obtained when a process is carried out reversibly in an isothermal process.

CO2 hydrogenation (the stoichiometry is 1:1:1:1) CO2 (g) + H2 (g) → CO (g) + H2O (g) Table 1. Thermodynamic data (T = 298 K) 1.png (a) (10 points) At 298 K and 1 atm, if the system initially only contains 1 mole of CO2 (g) and 1 mole of H2 (g), what will be the remaining amount of CO2 (g) after the reaction? And what will be the conversion of CO2 (g) after the reaction? (b) (10 points) At 298 K and 1 atm, if the system initially contains 1 mole of CO2 (g), 4 moles of H2 (g), 2 moles of CO (g), and 3 moles of H2O (g), will the reaction favor the formation of more products or more reactants? Please perform calculations to support your conclusion. (c) (10 points) If we want to increase the conversion of CO2 and H2, should we adjust the reaction pressure or the temperature? Why? If so, what pressure or temperature conditions would be needed to achieve approximately 10% CO2 conversion?

For an isothermal process of an ideal gas, which statement is correct? 

For a reversible adiabatic ideal gas compression, the temperature decreases.

For the reaction in Question 11, this pressure-induced shift occurs because changing pressure affects the equilibrium constant Kp. 

The van ’t Hoff equation is used to determine how temperature change affects the equilibrium constant Kp.

Dogs and cats are eukaryotic organisms.