# Given, the following reaction: Given:  ∆ H∘ = 109 kJ/mol B.E. of (N-N) = 163 kJ/mol B.E. of (N-H) = 391 kJ/mol B.E. of (H-H) = 436 kJ/mol Calculate the bond enthalpy of N = N. 1. 182 kJ/mol 2. 400 kJ/mol 3. 300 kJ/mol 4. 218 kJ/mol

Subtopic:  Thermochemistry |
72%
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The pair of isochoric among the transformation of state is:

1. K to L and L to M

2. L to M and N to K

3. L to M and M to N

4. M to N and N to K

Subtopic:  Classification of System, Extensive & Intensive Properties |
89%
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Reversible expansion of an ideal gas under isothermal and adiabatic conditions are as shown in the figure:

AB$\to$Isothermal expansion

AC$\to$Adiabatic expansion

Which of the following options is not correct?

1. $∆{S}_{isothermal}>∆{S}_{adiabatic}$

2. ${T}_{A}={T}_{B}$

3. ${W}_{isothermal}>{W}_{adiabatic}$

4. ${T}_{C}>{T}_{A}$

Subtopic:  2nd & 3rd Law of Thermodynamics |
53%
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NEET - 2019
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An ideal gas expands isothermally from  at 300 K against a constant pressure of . The work done by  the gas is:

 1 +270 kJ 2 –900 J 3 +900 kJ 4 –900 kJ
Subtopic:  First Law of Thermodynamics |
70%
From NCERT
NEET - 2019
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 1 Energy changes involved in a chemical reaction. 2 The extent to which a chemical reaction proceeds. 3 The rate at which a reaction proceeds. 4 The feasibility of a chemical reaction.
Subtopic:  Thermodynamics' Properties and process |
71%
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Consider the following reactions:

 (i) H+(aq) + OH-(aq) → H2O(l) ΔH = -x1 kJmol-1 (ii) H2(g) + 1/2O2(g) → H2O(l) ΔH = -x2 kJmol-1 (iii) CO2(g) + H2(g) → CO (g) + H2O(l) ΔH = -x3 kJmol-1 (iv) C2H2(g) + 5/2O2(g) →  2CO2 + H2O(l) ΔH = -x4 kJmol-1

Enthalpy of formation of H2O(l) is :

1. $-{x}_{3}$ $kJ$ $mo{l}^{-1}$

2. $-{x}_{4}$ $kJ$ $mo{l}^{-1}$

3. $-{x}_{1}$ $kJ$ $mo{l}^{-1}$

4. $-{x}_{2}$ $kJ$ $mo{l}^{-1}$

Subtopic:  Thermochemistry |
75%
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AIPMT - 2007
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The heat of combustion of carbon to CO2 is –393.5 KJ/mol. The heat released upon the formation of 35.2 g of CO2 from carbon and oxygen gas is:
1. –315 KJ
2. +315 KJ
3. –630 KJ
4. +630 KJ

Subtopic:  Thermochemistry |
73%
From NCERT
NEET - 2015
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If for a certain reaction ${∆}_{r}H$ is 30 kJ mol–1 at 450 K, the value of ${∆}_{r}S$ (in JK–1 mol–1) for which the same reaction will be spontaneous at the same temperature is:

1. 70

2. –33

3. 33

4. –70

Subtopic:  Spontaneity & Entropy |
69%
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NEET - 2020
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Identify the correct statement regarding entropy:

 1 At absolute zero of temperature, the entropy of all crystalline substances is taken to be zero 2 At absolute zero of temperature, the entropy of a perfectly crystalline substance is +ve 3 At absolute zero of temperature, the entropy of a perfectly crystalline substance is taken to be zero 4 At 0 °C , the entropy of a perfectly crystalline substance is taken to be zero
Subtopic:  2nd & 3rd Law of Thermodynamics |
65%
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AIPMT - 1998
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Following reaction occurs at ${25}^{\circ }C$ :

2NO(g) , (1 × 10-5   atm) + Cl2(g), ( 1×10-2 atm) ⇌ 2NOCl(g), ( 1×10- 2 atm) ∆Go   is-

1. -45.65 kJ

2. -28.53 kJ

3. -22.82 kJ

4. -57.06 kJ

Subtopic:  Gibbs Energy Change |
62%
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