NEET Gibbs Energy Change Practice Questions With Solutions

NEET Chemistry Gibbs Energy Change Practice Questions

Biology Physics

Question 1.

A process among the following shows decrease in entropy is :

A\(2 \text H \left(g\right)\rightarrow\text H_{2} \left(g\right)\)

BEvaporation of water

CExpansion of a gas at a constant temperature

DSublimation of solid to gas

Question 2.

For a given reaction, ∆H = 35.5 kJ mol^–1 and ∆S = 83.6 J K^–1 mol^–1. The reaction is spontaneous at: (Assume that ∆H and ∆S do not vary with temperature)

AT > 425K

BAll temperatures

CT > 298K

DT < 425K

Question 3.

The correct thermodynamic conditions for a spontaneous reaction at all temperatures is:

∆

H > 0 and

∆

S< 0

∆

H < 0 and

∆

S> 0

∆

H < 0 and

∆

S< 0

∆

H > 0 and

∆

S = 0

Question 4.

In which of the following reactions, the standard reaction entropy change

(∆ S^{0})

is positive, and standard Gibb's energy change

(∆ G^{0})

decreases sharply with increasing temperature?

AC(graphite) + \(\frac{1}{2}\)O₂(g) → CO(g)

BCO(g) + \(\frac{1}{2}\)O₂(g) → CO₂(g)

CMg(s) + \(\frac{1}{2}\)O₂(g) → MgO(s)

D\(\frac{1}{2}\)C(graphite) + \(\frac{1}{2}\)O₂(g) → \(\frac{1}{2}\)CO₂(g)

Question 5.

For vaporization of water at 1 atmospheric pressure, the values of ∆H and ∆S are 40.63 kJ mol^–1 and 108.8 JK^–1 mol^–1, respectively. The temperature when Gibbs energy change (∆G) for this transformation will be zero, is:

A393.4 K

B373.4 K

C293.4 K

D273.4 K

Question 6.

Standard entropies of X₂, Y₂ and XY₃ are 60, 40 and 50JK^-1mol^-1 respectively. For the reaction

\frac{1}{2} X_{2}

+

\frac{3}{2} Y_{2}

⇋

{XY}_{3}

;

∆ H

=

- 30

kJ

to be at equilibrium, the temperature should be:

A750 K

B1000 K

C1250 K

D500 K

Question 7.

Which of the following are not state functions? (I) q + W (II) q (III) W (IV) H - TS

A(I) and (IV)

B(II), (III) and (IV)

C(I), (II) and (III)

D(II) and (III)

Question 8.

Which of the following statements about the advantage of roasting sulphide ore before reduction is not true?

1.	Carbon and hydrogen act as suitable reducing agents for metal sulphides
2.	The \(\Delta_f G^0\) of the sulphide is greater than those for \(C S_2\) and \(\mathrm{H}_2 \mathrm{~S}\)
3.	The \(\Delta_f G^0\) is negative for roasting of sulphur ore to oxide.
4.	Roasting of the sulphide to the oxide is thermodynamically feasible

ACarbon and hydrogen act as suitable reducing agents for metal sulphides

BThe \(\Delta_f G^0\) of the sulphide is greater than those for \(C S_2\) and \(\mathrm{H}_2 \mathrm{~S}\)

CThe \(\Delta_f G^0\) is negative for roasting of sulphur ore to oxide.

DRoasting of the sulphide to the oxide is thermodynamically feasible

Question 9.

The enthalpy and entropy change for the reaction: Br₂ (l) + Cl₂ (g) →2BrCl(g), are 30kJ mol^-1 and 105 JK^-1 mol^-1 respectively. The temperature at which the reaction will be in equilibrium is:

A285.7 K

B273 K

C450 K

D300 K

Question 10.

The standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are –382.64 kJ mol^–1 and –145.6 JK^–1 mol^–1, respectively. Standard Gibbs energy change for the same reaction at 298 K is:

A–339.3 kJ mol^–1

B– 439.3 kJ mol^–1

C–523.2 kJ mol^–1

D–221.1 kJ mol^–1

Question 1.

2 Z n + O_{2} \to 2 Z n O

∆ G ° = - 616

J

2 Z n + S_{2} \to 2 Z n S

∆ G ° = - 293

J

S_{2} + 2 O_{2} \to 2 S O_{2}

∆ G ° = - 408 J

∆ G °

for the following reaction is:

2 Z n S + 3 O_{2} \to 2 Z n O + 2 S O_{2}

A-731 J

B-1317 J

C-501 J

D+731 J

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NEET Gibbs Energy Change Practice Questions With Solutions

NEET Chemistry Gibbs Energy Change Practice Questions

Question 1.

Question 2.

Question 3.

Question 4.

Question 5.

Question 6.

Question 7.

Question 8.

Question 9.

Question 10.

Question 1.

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