Chemical Thermodynamics Mock Tests

Given: C(s) + O₂(g) → CO₂(g), ΔH = -393.5 kJ; 2CO(g) + O₂(g) → 2CO₂(g), ΔH = -566.0 kJ. The enthalpy of formation of CO(g) is:

At what temperature will the reaction be at equilibrium if ΔH = −40.0 kJ/mol and ΔS = −80.0 J/(mol·K)? (Assume ΔH and ΔS are temperature independent)

For the reaction N₂(g) + 3H₂(g) → 2NH₃(g), the correct statement about entropy change is:

For a reaction to be spontaneous at all temperatures, which combination of ΔH and ΔS must hold?

The entropy change (ΔS) for the vaporization of a liquid is 108 J K⁻¹ mol⁻¹. If its enthalpy of vaporization is 30.8 kJ mol⁻¹, the boiling point of the liquid is:

At what temperature will the reaction 2NO(g) + O₂(g) → 2NO₂(g) be at equilibrium if ΔH = −114.2 kJ/mol and ΔS = −146 J/(mol·K)?

The enthalpy of neutralization of a strong acid by a strong base is −57.1 kJ/mol. The enthalpy of neutralization of HCN by NaOH will be:

For a reaction at 298 K, ΔH = −92.0 kJ/mol and ΔS = −198 J/(mol·K). The reaction will be spontaneous at: