Chemical Thermodynamics Mock Tests

Given: C(s) + O₂(g) → CO₂(g), ΔH = -393.5 kJ mol⁻¹; CO(g) + ½O₂(g) → CO₂(g), ΔH = -283.0 kJ mol⁻¹. The enthalpy of formation of CO(g) is:

Given: C(s) + O₂(g) → CO₂(g), ΔH = -393.5 kJ/mol 2CO(g) + O₂(g) → 2CO₂(g), ΔH = -566.0 kJ/mol What is the enthalpy of formation of CO(g) from C(s) and O₂(g)?

The enthalpy of combustion of carbon to CO₂ is -393.5 kJ mol⁻¹. The mass of carbon required to produce 1570 kJ of heat at STP is:

Which of the following statements is correct about the second law of thermodynamics?

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:

The heat of reaction at constant pressure (Delta H) is related to Delta E by:

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:

When 1 mole of an ideal gas at 25°C is expanded reversibly from 8 dm³ to 20 dm³, the value of q (heat absorbed) is: