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Under isothermal condition, a gas at 300 K expands from 0.1 L to 0.25 L against a constant external pressure of 2 bar. The work done by the gas is: [Given that 1 L bar=100 J]

1. 30 J

2. -30 J

3. 5 kJ

4. 25 J

Q257:

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Subtopic: 2nd & 3rd Law of Thermodynamics |

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Assuming each reaction is carried out in an open container for which of the following reaction(s) will ΔH=ΔE ?

1. $H_{2} (g) + B r_{2} (g) \to 2 H B r (g)$

2. $C (s) + 2 H_{2} O (g) \to 2 H_{2} (g) + C O_{2} (g)$

3. $P C l_{5} (g) \to P C l_{3} (g) + C l_{2} (g)$

4. $2 C O (g) + O_{2} (g) \to 2 C O_{2} (g)$

Q256:

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Subtopic: Thermodynamics' Properties and process |

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

1. Carbon and hydrogen act as suitable reducing agents for metal sulphides

2. The $∆_{f} G^{0}$ of the sulphide is greater than those for $C S_{2}$ and $H_{2} S$

3. The $∆_{f} G^{0}$ is negative for roasting of sulphur ore to oxide.

4. Roasting of the sulphide to the oxide is thermodynamically feasible

Q255:

From NCERT AIPMT - 2007

Subtopic: Gibbs Energy Change | Hess's Law |

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The bond energy of H—H and Cl-Cl is 430 kJ mol^-1 and 240 kJ mol^-1 respectively and ΔH_f for HCl is -90 kJ mol^-1. The bond enthalpy of HCl is :

1. 290 $k J m o l^{- 1}$

2. 380 $k J m o l^{- 1}$

3. 425 $k J m o l^{- 1}$

4. 245 $k J m o l^{- 1}$

Q254:

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Subtopic: Thermochemistry |

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Bond dissociation enthalpy of H₂, Cl₂ and HCl are 434, 242 and 431 kJ mol¹ respectively. Enthalpy of formation of HCl is

1. 93 kJ mol^-1
2. - 245 kJ mol^-1
3. -93 kJ mol^-1
4. 245 kJ mol^-1

Q253:

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Subtopic: Thermochemistry |

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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 E_cell for the pentane-oxygen fuel cell is:

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

Q252:

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Subtopic: Gibbs Energy Change |

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For the gas phase reaction,

{PCl}_{5} (g) ⇌ {PCl}_{3} (g) + {Cl}_{2} (g)

which of the following conditions are correct?

1. ΔH = 0 and ΔS < 0

2. ΔH > 0 and ΔS > 0

3. ΔH < 0 and ΔS < 0

4. ΔH > 0 and ΔS < 0

Q251:

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Subtopic: Gibbs Energy Change |

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The values of ΔH and ΔS for the reaction, C_(graphite) + CO₂(g)→2CO(g) are 170 kJ and 170 JK^-1, respectively. This reaction will be spontaneous at
1. 710 K
2. 910 K
3. 1110 K
4. 510 K

Q250:

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Subtopic: Gibbs Energy Change |

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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

Q249:

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Subtopic: Thermochemistry |

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In which case, change in entropy is negative?

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2. Evaporation of water

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4. Sublimation of solid to gas

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In which case, change in entropy is negative? 1. 2Hg → H2g 2. Evaporation of water 3. Expansion of a gas at a constant temperature 4. Sublimation of solid to gas

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In which case, change in entropy is negative?

1. $2 H (g) \to H_{2} (g)$

2. Evaporation of water

3. Expansion of a gas at a constant temperature

4. Sublimation of solid to gas