Which, among the following, is not a state function?

1. Internal energy

2. Free energy

3. Work

4. Enthalpy

Subtopic:  Thermodynamics' Properties and process |
 88%
From NCERT
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NEET 2023 - Target Batch - Aryan Raj Singh
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NEET 2023 - Target Batch - Aryan Raj Singh

Which of the following is correct for isothermal expansion of an ideal gas -

1. Wrev = Wirr

2. Wrev + Wirr = 0

3. Wrev > Wirr

4. qrev = qirr

Subtopic:  First Law of Thermodynamics |
 67%
From NCERT
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NEET 2023 - Target Batch - Aryan Raj Singh
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Which among the following state functions is an extensive property of the system?

1. Temperature 2. Volume
3. Refractive index 4. Viscosity
Subtopic:  Classification of System, Extensive & Intensive Properties |
 78%
From NCERT
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The correct statement for a reversible process in a state of equilibrium is:
1. G = - 2.30RT log K
2. G = 2.30RT log K
3. Go = - 2.30RT log K
4. Go = 2.30RT log K

Subtopic:  Gibbs Energy Change |
 78%
From NCERT
NEET - 2015
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Given the Gibbs free energy change, \(\Delta G^\circ=+63.3~kJ,\) for the following reaction, 
\(Ag_2 CO_3 (g) \rightarrow 2Ag^+ (aq) + CO^{2-}_3 (aq)\)
\(K_{sp}\) of \(Ag_2CO_3 (s) \) in water at 25º C is (R = 8.314 JK-1 mol-1)

1. \(3.2 \times 10^{26}\)
2. \(8.0 \times 10^{-12}\)
3. \(2.9 \times 10^{-3}\)
4. \(7.9 \times 10^{-2}\)
Subtopic:  Gibbs Energy Change |
 60%
From NCERT
AIPMT - 2014
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Which of the following statements is correct for the spontaneous adsorption of a gas?

1. ∆ S is negative and therefore,  ∆ H should be highly positive
2. ∆ S is negative and therefore,  ∆ H should be highly negative
3. ∆ S is positive and therefore,  ∆ H should be negative
4. -∆ S is positive and therefore,  ∆ H should also be highly positive

Subtopic:  Spontaneity & Entropy |
 57%
From NCERT
AIPMT - 2014
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Given the following reaction:
\(4H(g)\)→  \(2 H_{2}\)\((g)\)
The enthalpy change for the reaction is -869.6 kJ. The dissociation energy of the H-H bond is:
1. -869.6 kJ
2. +434.8kJ
3. +217.4kJ
4. -434.8 kJ

Subtopic:  Enthalpy & Internal energy |
 68%
From NCERT
AIPMT - 2011
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From the following bond energies:
H—H bond energy: 431.37 kJ mol-1 
C=C bond energy: 606.10 kJ mol-1 
C—C bond energy: 336.49 kJ mol-1 
C—H bond energy: 410.50 kJ mol-1 
Enthalpy for the reaction, 

will be:

1. 1523.6 kJ mol-1 2. -243.6 kJ mol-1
3. -120.0 kJ mol-1 4. 553.0 kJ mol-1
Subtopic:  Thermochemistry |
 75%
From NCERT
AIPMT - 2009
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The values of ΔH and ΔS for the given reaction are 170 kJ and 170 JK-1, respectively.
C(graphite) + CO2(g)→2CO(g) 
This reaction will be spontaneous at:

1. 710 K
2. 910 K
3. 1110 K
4. 510 K

Subtopic:  Gibbs Energy Change |
 88%
From NCERT
AIPMT - 2009
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The standard free energies of formation(in kJ/mol) at 298 K are -237.2, -394.4, and -8.2 for H2O(l), CO2(g), and pentane (g), respectively. The value of Ecell for the pentane-oxygen fuel cell is:

1. 1.968 V
2. 2.0968 V
3. 1.0968 V
4. 0.0968 V

Subtopic:  Gibbs Energy Change |
 55%
From NCERT
AIPMT - 2008
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