Thermodynamics Mock Tests

The entropy of a perfectly crystalline substance at 0 K is zero. This is:

Given: C(s) + O₂(g) → CO₂(g), ΔH = −393.5 kJ/mol; H₂(g) + ½O₂(g) → H₂O(l), ΔH = −285.8 kJ/mol; C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(l), ΔH = −2220.0 kJ/mol. The standard enthalpy of formation of C₃H₈(g) is:

Given: ΔHf°(H₂O, l) = −286 kJ mol⁻¹, ΔHvap(H₂O) = +44 kJ mol⁻¹, bond enthalpies: H−H = 436 kJ mol⁻¹, O=O = 498 kJ mol⁻¹. Calculate the O−H bond enthalpy.

The first law of thermodynamics is essentially a statement of conservation of:

An ideal gas expands isothermally from volume V₁ to volume V₂. The work done by the gas is:

Mean free path of gas molecules is inversely proportional to:

A heat engine absorbs 500 J of heat from a hot reservoir at 400 K and rejects 300 J to a cold reservoir. The efficiency of the engine is:

An ideal gas is taken through a cyclic process ABCA as shown on a P-V diagram. The net work done by the gas in one cycle is: