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Thermodynamics — JEE Chemistry MCQs

Master Thermodynamics for JEE Main with free chemistry MCQs. Each question includes a detailed solution and instant feedback — practice at easy, medium, and hard difficulty levels to build exam-ready confidence.

12 practice questions with instant feedback and solutions.

Easy•Thermodynamics
For an exothermic reaction at constant pressure, which of the following is true?
Easy•Thermodynamics
In an isothermal expansion of an ideal gas, 500 J of heat is absorbed by the system. The work done by the gas is:
Easy•Thermodynamics
The enthalpy of combustion of methane is −890-890 kJ/mol. If 88 g of methane is completely burnt, the heat released is (Molar mass of CH₄ = 16 g/mol):
Medium•Thermodynamics
Given the following thermochemical equations: - C(s) + O₂(g) → CO₂(g); ΔH₁ = -393 kJ/mol - CO(g) + ½O₂(g) → CO₂(g); ΔH₂ = -283 kJ/mol The enthalpy of formation of CO(g) is:
Medium•Thermodynamics
For a reaction to be spontaneous at all temperatures, which of the following conditions must be satisfied?
Easy•Thermodynamics
Two moles of an ideal gas undergo a reversible isothermal expansion at 300 K, where the volume increases from 10 L to 20 L. The work done by the gas is (R = 8.314 J/mol·K, ln 2 = 0.693):
Easy•Thermodynamics
For vaporization of 11 mole of water at 100°C100°C and 11 atm, if ΔHvap=40.7\Delta H_{vap} = 40.7 kJ/mol, the entropy change is:
Hard•Thermodynamics
The standard state Gibbs free energies of formation of C\mathrm{C} (graphite) and CC (diamond) at T=298 K\mathrm{T}=298 \mathrm{~K} are ΔfGo[C( graphite )]=0 kJ molΔfGo[C( diamond )]=2.9 kJ mol−1. \begin{gathered} \Delta_{f} G^{o}[\mathrm{C}(\text { graphite })]=0 \mathrm{~kJ} \mathrm{~mol} \\ \Delta_{f} G^{o}[\mathrm{C}(\text { diamond })]=2.9 \mathrm{~kJ} \mathrm{~mol}^{-1} . \end{gathered} The standard state means that the pressure should be 1 bar, and substance should be pure at a given temperature. The conversion of graphite [ C(graphite)] to diamond [ C(diamond)] reduces its volume by 2×10−6 m3 mol−12 \times 10^{-6} \mathrm{~m}^{3} \mathrm{~mol}^{-1}. If C\mathrm{C} (graphite) is converted to C\mathrm{C} (diamond) isothermally at T=298 K\mathrm{T}=298 \mathrm{~K}, the pressure at which C\mathrm{C} (graphite) is in equilibrium with C(\mathrm{C}( diamond), is [Useful information: 1 J=1 kg m2 s−2;1 Pa=1 kg m−1 s−2;11 \mathrm{~J}=1 \mathrm{~kg} \mathrm{~m}^{2} \mathrm{~s}^{-2} ; 1 \mathrm{~Pa}=1 \mathrm{~kg} \mathrm{~m}^{-1} \mathrm{~s}^{-2} ; 1 bar =105 Pa=10^{5} \mathrm{~Pa} ]
Medium•Thermodynamics
Using the bond enthalpies: C-H = 414414 kJ/mol, C-C = 347347 kJ/mol, C=C = 611611 kJ/mol, H-H = 435435 kJ/mol. The enthalpy change for the hydrogenation of ethene (C2H4+H2→C2H6\text{C}_2\text{H}_4 + \text{H}_2 \rightarrow \text{C}_2\text{H}_6) is:
Medium•Thermodynamics
One mole of an ideal gas at 300 K300 \mathrm{~K} in thermal contact with surroundings expands isothermally from 1.0 L1.0 \mathrm{~L} to 2.0 L2.0 \mathrm{~L} against a constant pressure of 3.0 atm3.0 \mathrm{~atm}. In this process, the change in entropy of surroundings (ΔSsurr )\left(\Delta S_{\text {surr }}\right) in JK−1\mathrm{J} \mathrm{K}^{-1} is (1 Latm⁡=101.3 J)\mathrm{L} \operatorname{atm}=101.3 \mathrm{~J})
Medium•Thermodynamics
One mole of an ideal monoatomic gas at 300 K expands irreversibly and isothermally from 10 L to 20 L against a constant external pressure of 1 atm. The entropy change of the universe is (R = 8.314 J/mol·K, ln 2 = 0.693, 1 L·atm = 101.3 J):
Medium•Thermodynamics
One mole of an ideal monoatomic gas (γ = 5/3) undergoes a reversible adiabatic expansion from initial temperature 400 K and volume 2 L to final volume 16 L. The final temperature of the gas is:
Thermodynamics JEE Chemistry MCQs — Practice Questions | MyGoalPrep