Theromodynamics and Thermochemistry Test

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Theromodynamics and Thermochemistry Test - 6

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Weekly Quiz Competition

Question 1
1 / -0

For the reaction
X₂O₄ (η) →2XO₂ (g) ΔE = 2.1 kcal,
ΔS = 20 cal/K at 300 K. Hence ΔG is–

A
2.7 kcal

B
– 2.7 kcal

C
9.3 kcal

D
– 9.3 kcal

Solution

From ΔH = ΔE + ΔnRT
ΔH = 2.1 + 2 × (2 × 10^–3) × 300
= 3.3
Now from ΔG = ΔH – TΔS
= 3.3 – 300 × (20 × 10^–3)
= – 2.7 k cal
Question 2
1 / -0

When one mole of uni-univalent salt AB is dissolved in water at 300 K, 3.7 kJ of heat is absorbed but ΔG of the process is – 8.3 kJ. What is the value of ΔS for the dissolution process ?

A
40 JK^–1

B
30 JK^–1

C
20 JK^–1

D
– 15.3 JK^–1

Solution

Given, T = 300 K, ΔH = 3.7 kJ
ΔG = – 8.3 kJ, ΔS = ?
From ΔG = ΔH – TΔS
⇒– 8.3 = 3.7 – 300 × ΔS
⇒ΔS = 0.04
= 40 JK–1
Question 3
1 / -0

Which of the following process/es proceed towards more disordered state?
I. stretching the
II. Sublimation of rubber dry ice
III. Crystallisation of
IV. dissolution of salt from solution sugar from solution

A
I, II, IV

B
I, III

C
III, IV

D
II, IV

Solution

In I & IV entropy increases due to increase in randomness.
Question 4
1 / -0

When ice melts into water, entropy -

A
Becomes zero

B
Decreases

C
Increases

D
Remains same

Solution

Entropy will be increases
Question 5
1 / -0

In which of the following reactions ΔS is positive?

A
H₂O (l) → H₂O (s)

B
3O₂ (g) → 2O₃ (g)

C
H₂O (l) → H₂O (g)

D
N₂(g) + 3H₂ (g) → 2NH₃(g)

Solution

ΔS = ∑nΔs (Products) – ∑n Δs (Reactants)
In option C. entropy change is +ve as gases have higher entropy as compared to liquids.

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Theromodynamics and Thermochemistry Test - 6

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Theromodynamics and Thermochemistry Test - 6

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Question 1

2.7 kcal

– 2.7 kcal

9.3 kcal

– 9.3 kcal

Solution

Question 2

40 JK–1

30 JK–1

20 JK–1

– 15.3 JK–1

Solution

Question 3

I, II, IV

I, III

III, IV

II, IV

Solution

Question 4

Becomes zero

Decreases

Increases

Remains same

Solution

Question 5

H2O (l) → H2O (s)

3O2 (g) → 2O3 (g)

H2O (l) → H2O (g)

N2(g) + 3H2 (g) → 2NH3(g)

Solution

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40 JK^–1

30 JK^–1

20 JK^–1

– 15.3 JK^–1

H₂O (l) → H₂O (s)

3O₂ (g) → 2O₃ (g)

H₂O (l) → H₂O (g)

N₂(g) + 3H₂ (g) → 2NH₃(g)