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NEET UG Thermodynamics — practice questions — page 3

Explore 95 free Thermodynamics questions in NEET UG Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Thermodynamics questions and exercises with answers

Showing questions 61–90 of 95.

Since ∆solH is positive for most ionic compounds, their solubility in water:Read the answer and worked solution →If the lattice enthalpy of an ionic compound is very high, then the compound:Read the answer and worked solution →At temperature T, ionization enthalpy relates to ionization energy E0 as:Read the answer and worked solution →Enthalpy of solution refers to one mole dissolving in:Read the answer and worked solution →HCl(g) + 10 aq has ∆H -69.01; + 25 aq has -72.03 kJ/mol. ∆H of HCl.10aq + 15 aq?Read the answer and worked solution →In thermodynamics, calling a process spontaneous means it:Read the answer and worked solution →Why can a fall in enthalpy not alone decide spontaneity?Read the answer and worked solution →Two gases mix in an isolated box with ∆H = 0. What drives the mixing?Read the answer and worked solution →Entropy can be pictured as a measure of a system's:Read the answer and worked solution →For a given substance, which state has the lowest entropy?Read the answer and worked solution →For a reversible process at temperature T, the entropy change is given by:Read the answer and worked solution →For isothermal ideal gas expansion, which quantity tells reversible from irreversible paths?Read the answer and worked solution →In which change does the entropy of the system decrease?Read the answer and worked solution →At 298 K, 4Fe + 3O2 → 2Fe2O3 has ∆rS = -549.4 J/K mol and ∆rH = -1648 kJ/mol. ∆Stotal?Read the answer and worked solution →At temperature T, the entropy change of the surroundings for a reaction is:Read the answer and worked solution →Which expression defines the Gibbs energy, G?Read the answer and worked solution →At constant temperature and pressure, a process is spontaneous when ∆G is:Read the answer and worked solution →∆G is a valid criterion for spontaneity under conditions of constant:Read the answer and worked solution →∆G is called the free energy because it represents the energy:Read the answer and worked solution →A reaction with negative ∆H and positive ∆S is spontaneous:Read the answer and worked solution →A reaction has ∆H = +40 kJ/mol and ∆S = +100 J/K mol. It becomes spontaneous above:Read the answer and worked solution →For a reaction at 300 K, ∆H = -10 kJ/mol and ∆S = -20 J/K mol. What is ∆G?Read the answer and worked solution →The second law of thermodynamics says that in an isolated system a spontaneous change is marked by:Read the answer and worked solution →The third law says entropy approaches zero at absolute zero for any:Read the answer and worked solution →At equilibrium at constant T and p, the Gibbs energy change of a reaction is:Read the answer and worked solution →Standard Gibbs energy change and the equilibrium constant K are related by:Read the answer and worked solution →For a strongly exothermic reaction with large negative ∆rG°, the value of K is:Read the answer and worked solution →A reaction has K = 10 at 300 K. Using R = 8.314 J/K mol, ∆rG° is about:Read the answer and worked solution →Kp for 3/2 O2(g) → O3(g) at 298 K is 2.47 x 10^-29. ∆rG° for this change is about:Read the answer and worked solution →Two moles of ideal gas expand reversibly at 300 K to ten times their volume. Work done w?Read the answer and worked solution →

Worked practice questions

Since ∆solH is positive for most ionic compounds, their solubility in water:

  1. Is zero at room temperature
  2. Ignores temperature
  3. Rises with temperature
  4. Falls with temperature
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Correct answer: C. Rises with temperature

Endothermic dissolution is favoured by heating, so most salts dissolve more at higher temperature.

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If the lattice enthalpy of an ionic compound is very high, then the compound:

  1. May not dissolve at all
  2. Dissolves very quickly
  3. Melts at a low temperature
  4. Dissolves with heat release
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Correct answer: A. May not dissolve at all

A very large lattice enthalpy cannot be offset by hydration, so dissolution may not happen.

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At temperature T, ionization enthalpy relates to ionization energy E0 as:

  1. E0 + RT
  2. E0 + 5/2 RT
  3. E0 - 5/2 RT
  4. E0 + 3/2 RT
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Correct answer: B. E0 + 5/2 RT

Ionization creates an extra gaseous particle with Cp = 5/2 R, adding 5/2 RT to the 0 K energy.

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