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Chemical Thermodynamics MCQs for NEET — Chemistry Questions with Answers

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At 1000 K water vapour at 1 atm. has been found to be dissociated into H₂ and O₂ to the extent of 3 x 10^–6 %.Calculate the free energy decrease of the system, assuming ideal behaviour.

–ΔG = 90,060 cal

–ΔG = 20 cal

–ΔG = 480 cal

–ΔG = –45760 cal

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Explanation

H₂O(g) $\overset{}{⇌}$ H₂O + $\frac{1}{2}$ O₂

1 – α α α/2

K_P = $\frac{α \times {(α / 2)}^{1 / 2}}{(1 - α)}$ × $\frac{P}{(1 + \frac{α}{2})}$ = 11.62 × 10–11 (atm)^1/2

ΔG° = – RT In K_p = – 45.76 kcal

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When 1 mole of an ideal gas at 20 atm pressure and 15 L volume expands such that the final pressure becomes 10 atm and the final volume become 60 L. Calculate entropy change for the process (C_pm = 30.96 J mole^–1 K^–1)

80.2 J.k^–lmo1^–1

62.42 kJ.k^–1 mol^–1

120 x 10² J1c¹mol^–1

27.22 J.k^–1mor

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Explanation

$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$

$\frac{T_{2}}{T_{1}} = \frac{6}{3}$

ΔS = 2.303 × n $\{C_{p} \log_{10} \frac{T_{2}}{T_{1}} + R \log_{10} \frac{P_{1}}{P_{2}}\}$

ΔS = 2.303 × 1 $\{10 .96 \log_{10} \frac{6}{3} + R \log_{10} \frac{20}{10}\}$

ΔS = 27.22 J.K^–1 mol^–1

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During winters, moisture condenses in the form of dew and can be seen on plant leaves and grass. The entropy of the system in such cases decreases as liquids possess lesser disorder as compared to gases. With reference to the second law, which statement is correct, for the above process ?

The randomness of the universe decreases

The randomness of the surroundings decreases

Increase is randomness of surroundings equals the decrease in randomness of system

The increase in randomness of the surroundings is greater as compared to the decrease in randomnessof the system.

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Explanation

As dew formation is spontaneous process therefore entropy or randomness of the universe will increase. As randomeness of system has decreased but randomness of the surrounding will increase larger so that change is positive.

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For which process will $∆$ H° and $∆$ G° be expected to be most similar.

2Al(s) + Al₂O₃(s) → 2Fe(s) + A_l2O₃(s)

2Na(s) + 2H₂O(l) → 2NaOH(aq) + H₂(g)

2NO₂(g) → N₂O₄(g)

2H₂(g) + O₂(g) → 2H₂O(g)

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Explanation

All product and reactants are in solid state

So ΔS° ≈ 0

ΔG° = ΔH – TΔS°

So ΔG° ≈ ΔH°

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Heat produced in calories by the combustion of one gram of carbon is called

Heat of combustion of carbon

Heat of formation of carbon

Calorific value of carbon

Heat of production of carbon

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Explanation

It is the definition of calorific value.

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For the isothermal expansion of an ideal gas

E and H increases

E increases but H decreases

H increases but E decreases

E and H are unaltered

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Explanation

In isothermal reversible process ideal gas has constant temperature and so ΔE = 0 and ΔH = ΔE = 0.

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If a refrigerator's door is opened, then we get [CPMT 1980]

Room heated

Room cooled

More amount of heat is passed out

No effect on room

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Explanation

The compressor has to run for longer time releasing more heat to the surroundings.

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Point out the wrong statement in relation to enthalpy

It is a state function

It is an intensive property

It is independent of the path followed for the change

Its value depends upon the amount of substance in the system

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Explanation

Enthalpy is an extensive property.

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Mark the correct statement

For a chemical reaction to be feasible, ΔG should be zero

Entropy is a measure of order in a system

For a chemical reaction to be feasible, ΔG should be positive

The total energy of an isolated system is constant

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Explanation

Total energy of an isolated system is constant.

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Internal energy is an example of [Pb. PMT 2000]

Path function

State function

Both (1) and (2)

None of these

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Explanation

The functions whose value depends only on the state of a system are known as state functions.

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