Author: Anonymous

For an ideal gas, the Joule–Thomson coefficient is zero. 

1. A system absorbs 500 J of heat from the surroundings, and the surroundings do 300 J of work on the system. What is the change in internal energy of the system? 

For CO(g) + 1/2 O2(g) → CO2(g), ΔH is the enthalpy of formation of CO2(g). 

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

Carnot cycle only contains isothermal and adiabatic processes. 

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?

Use thermodynamic relationships to fill in the blanks: (∂G/∂P)T = ______, (∂H/∂S)P = ______

Which of the following processes produces a decrease in the entropy of the system? 

The half-life of a certain zero-order reaction is constant.

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