List of top Chemistry Questions on Work done in Thermodynamics

The work done by a gas during an isothermal expansion from 2 L to 4 L at a constant temperature, with pressure initially at 2 atm, is: (Use R = 8.314 J/mol·K, T = 300 K).
For the reaction CO(g) + (1)/(2)textO₂(textg) → textCO₂(textg), which one of the statements is correct at constant T and P?
For a given reaction, Δ H = 35.5kJ mol⁻1 and Δ S = 83.6J K⁻1mol⁻1. The reaction is spontaneous at (Assume that Δ H and Δ S do not vary with temperature)
For a particular reversible reaction at temperature T, Δ H and Δ S were found to be both positive. If Tₑ is the temperature at equilibrium, then the reaction would be spontaneous when:
A spontaneous reaction is impossible if
Which law of thermodynamics helps in calculating the absolute entropies of various substances at different temperatures?
For vaporization of water at 1 atmospheric pressure, the values of Δ H and Δ S are 40.63kJ mol⁻1 and 108.8J K⁻1mol⁻1, respectively. The temperature when Gibbs free energy change (Δ G) for this transformation will be zero, is:
For a given reaction, Δ H = 35.5 kJ mol^-1 and Δ S = 83.6 J K⁻1 mol⁻1. The reaction is spontaneous at
For the reaction CO(g) + (1)/(2)O₂(g) → CO₂(g), which one of the statements is correct at constant T and P?

Figure below shows two paths that may be taken by a gas to go from a state A to a state C. In process AB, 400J of heat is added to the system and in process BC, 100J of heat is added to the system. The heat absorbed by the system in the process AC will be: 

For a particular reversible reaction at temperature T, Δ H and Δ S were found to be both positive. If Tₑ is the temperature at equilibrium, the reaction would be spontaneous when:
A spontaneous reaction is impossible if:
Which law of thermodynamics helps in calculating the absolute entropies of various substances at different temperatures?
If the enthalpy of vaporization of water is \(18.6\,\text{kJ mol}^{-1}\), the entropy of its vaporization will be:
The enthalpy of combustion of 2 moles of benzene at 27°C differs from the value determined in bomb calorimeter by
What is the free energy change, Δ G, when 1.0 mole of water at 100C and 1 atm pressure is converted into steam at 100C and 1 atm pressure?