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The heat of combustion of carbon to CO_{2} is –393.5 KJ/mol. The heat released upon the formation of 35.2 g of CO_{2} 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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The correct statement for a reversible process in a state of equilibrium is:

1. $\u2206$G = – 2.30RT log K

2. $\u2206$G = 2.30RT log K

3. $\u2206$G^{o} = – 2.30RT log K

4. $\u2206$G^{o} = 2.30RT log K

Subtopic: Gibbs Energy Change |

79%

From NCERT

NEET - 2015

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Given the Gibbs free energy change, \(\Delta \text G^\circ=+63.3~\text{kJ},\) for the following reaction,

\(\mathrm{Ag_2 CO_3 (g) \rightarrow 2Ag^+ (aq) + CO^{2-}_3 (aq)}\)

\(\mathrm{K_{sp}}\) of \(\mathrm {Ag_2CO_3 (s) }\) 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. \(7.9 \times 10^{-2}\)

\(\mathrm{Ag_2 CO_3 (g) \rightarrow 2Ag^+ (aq) + CO^{2-}_3 (aq)}\)

\(\mathrm{K_{sp}}\) of \(\mathrm {Ag_2CO_3 (s) }\) in water at 25º C is (R = 8.314 JK

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 |

56%

From NCERT

AIPMT - 2014

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Given the reaction:

X_{2}O_{4}(l) → 2XO_{2}(g)

ΔU = 2.1 kcal, ΔS = 20 cal K^{–1} at 300 K

The value of ΔG is:

1. 2.7 kcal

2. –2.7 kcal

3. 9.3 kcal

4. –9.3 kcal

Subtopic: Gibbs Energy Change |

78%

From NCERT

AIPMT - 2014

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When 5 litres of a gas mixture of methane and propane is perfectly combusted at 0°C and 1 atmosphere, 16 litres of oxygen at the same temperature and pressure is consumed. The amount of heat released from this combustion in kJ (\(\Delta \)H_{comb}. (CH_{4}) = 890 kJ mol^{–1}, \(\Delta \)H_{comb}( C_{3}H_{8}) = 2220 kJ mol^{–1}) is:

1. 38

2. 317

3. 477

4. 32

1. 38

2. 317

3. 477

4. 32

Subtopic: Thermochemistry |

60%

From NCERT

NEET - 2013

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Three thermochemical equations are given below:

Based on the above equations, find out which one of the relationships given below is correct :

(i) | C_{(graphite)} + O_{2}(g) \(\rightarrow\) CO_{2}(g); \(\Delta_{r}\)H° = x kJ mol^{–1} |

(ii) | C_{graphite} + 1/2 O_{2}(g) \(\rightarrow\) CO(g); \(\Delta_{r}\)H° = y kJ mol^{–1} |

(iii) | CO(g) + 1/2 O_{2}(g) \(\rightarrow\) CO_{2}(g); \(\Delta_{r}\)H° = z kJ mol^{–1} |

1. | z = x + y | 2. | x = y + z |

3. | y = 2z – x | 4. | x = y – z |

Subtopic: Hess's Law |

78%

From NCERT

NEET - 2013

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

$(\u2206{S}^{0})$ is positive, and standard Gibb's energy change

$(\u2206{G}^{0})$ decreases sharply with increasing temperature?

1. | C(graphite) + \(\frac{1}{2}\)O_{2}(g) → CO(g) |

2. | CO(g) + \(\frac{1}{2}\)O_{2}(g) → CO_{2}(g) |

3. | Mg(s) + \(\frac{1}{2}\)O_{2}(g) → MgO(s) |

4. | \(\frac{1}{2}\)C(graphite) + \(\frac{1}{2}\)O_{2}(g) → \(\frac{1}{2}\)CO_{2}(g) |

Subtopic: Gibbs Energy Change |

69%

From NCERT

AIPMT - 2012

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The enthalpy of fusion of water is 1.435 kcal/mol. The molar entropy change for the melting of ice at 0 ^{o}C is:

1. 10.52 cal/(mol K)

2. 21.04 cal/(mol K)

3. 5.260 cal/(mol K)

4. 0.526 cal/(mol K)

Subtopic: Thermochemistry |

79%

From NCERT

AIPMT - 2012

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The standard enthalpy of vaporization ${\u2206}_{\mathrm{vap}}{\mathrm{H}}^{\mathrm{o}}$ for water at 100 ^{o}C is 40.66 kJ mol^{-1}.

The internal energy of vaporization of water at 100 ^{o}C (in kJ mol^{-1}) is:

(Assume water vapour behaves like an ideal gas.)

1. +37.56

2. -43.76

3. +43.76

4. +40.66

Subtopic: Enthalpy & Internal energy |

59%

From NCERT

AIPMT - 2012

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