NCERT/Class 11/Chemistry/Thermodynamics

Thermodynamics

Class 11 · Chemistry

64 questions22 easy30 medium12 hard

Sample Questions

Q1.Which of the following correctly represents an adiabatic process?

  • Aq = 0 (no heat exchange with surroundings)
  • BΔT = 0 (no temperature change)
  • CΔU = 0 (no internal energy change)
  • DΔH = 0 (no enthalpy change)

Q2.The enthalpy of neutralization of a strong acid by a strong base is approximately:

  • A-57.1 kJ/mol
  • B+57.1 kJ/mol
  • C-100 kJ/mol
  • D0 kJ/mol

Q3.Kirchhoff's equation relates the change in enthalpy with temperature as:

  • AΔH(T₂) = ΔH(T₁) + ΔCp(T₂ - T₁)
  • BΔH(T₂) = ΔH(T₁) - ΔCp(T₂ - T₁)
  • CΔH(T₂) = ΔH(T₁) × ΔCp
  • DΔH(T₂) = ΔH(T₁)/T₁

Q4.The internal energy of an ideal gas depends on:

  • ATemperature only
  • BPressure only
  • CVolume only
  • DBoth pressure and temperature

Q5.In which of the following cases is ΔH approximately equal to ΔU?

  • AReactions in solution (condensed phase)
  • BReactions involving many moles of gases
  • CReactions at very high temperatures
  • DReactions with large Δng

Q6.This is a sample question to preview what you'll get in the full practice test...

  • A. Option one
  • B. Option two
  • C. Option three
  • D. Option four
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Concepts Covered

Boltzmann entropyBorn-Haber cycleCO2Cp vs CvFaraday's constantGibbs energyGibbs energy analysisGibbs free energyGibbs free energy criterionH and S relationshipH2O entropyHess's lawHess's law calculationHess's law manipulationsJoule's lawK = 1K > 1Kirchhoff's equationMayer's relationNH4NO3 dissolutionNaClPV workPV work negligibleadiabatic processamount of matterbenzene stabilitybomb calorimeterbond breaking and formingbond dissociation energybond enthalpybond enthalpy calculationcalorimetercombustion enthalpycombustion reactioncondensed phase reactionsconservation of energyconstant T and Pconstant external pressureconstant pressureconstant temperatureconstant valueconstant volumecrossover temperaturedefinitiondisorderdissolutionelectrochemical cellselectronic transitionsendothermicendothermic reactionendothermic spontaneityenergy conservationenthalpyenthalpy calculationenthalpy changeenthalpy measuremententhalpy of atomizationenthalpy of combustionenthalpy of neutralizationenthalpy of solutionenthalpy of sublimationenthalpy variation with temperatureentropyentropy at 0 Kentropy changeentropy comparisonentropy decreaseentropy definitionentropy driven dissolutionentropy of fusionentropy of gasesentropy of precipitationentropy of universeentropy-driven processequilibrium conditionequilibrium constantequilibrium constant from ΔG°equilibrium statesexothermic reactionextensive propertiesfirst lawfirst law of thermodynamicsfree expansionfuelsgas phase reactiongraphiteheat absorptionheat capacityheat capacity differenceheat exchangeideal gasideal gas internal energyinfinite dilutionintensive propertiesinternal energyions to solidisothermal processlatent heatlattice enthalpymatter and energy exchangemaximum workmeltingmelting point equilibriummicrostatesnon-spontaneityoctaneopen systempath functionperfect crystalphase transitionphase transitionsphoton energyreaction enthalpyreduction in gas molesreference stateresonance energyreverse reactionreversible isothermal expansionreversible processreversing and scalingreversing equationssecond lawsecond law of thermodynamicssign of ΔHspontaneityspontaneity at all temperaturesspontaneity calculationspontaneity conditionsspontaneity thresholdspontaneous processesspontaneous reactionstandard Gibbs energystandard conditionsstandard enthalpy of formationstandard statestandard statesstate functionstates of matterstrong acid-basesystem boundarytemperature dependencethermodynamic surroundingsthermodynamic systemsthird law of thermodynamicsuniversevacuum expansionwork = 0work calculationwork done in expansionΔG = 0ΔG = ΔH - TΔSΔG calculationΔG° and KΔG° and K relationshipΔG° and emfΔH < 0 ΔS > 0ΔH = ΔU conditionΔH > 0ΔH > 0 ΔS < 0ΔH sign conventionΔH vs ΔUΔH ≈ ΔU conditionΔS = ΔH/TΔU measurementΔfH° of methaneΔng = 0Δng calculationΔng relationship

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