What is the change in Gibbs free energy (ΔG) for the melting of three moles of water at 0°C?

1.	Zero	2.	Positive
3.	Negative	4.	Unpredictable

Subtopic: Gibbs Energy Change |

Level 3: 35%-60%

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Q2:

Given :

$C_{(Graphite)} + O_{2} (g) \to {CO}_{2} (g);$
$∆_{r} H ° = - 393.5 {KJmol}^{- 1};$
$H_{2} (g) + \frac{1}{2} O_{2} (g) \to H_{2} O (I);$
$∆_{r} H ° = - 285.8 KJ {mol}^{- 1};$
${CO}_{2} (g) + 2 H_{2} O (I) \to {CH}_{4} (g) + 2 O_{2} (g);$
$∆_{r} H ° = + 890.3 KJ {mol}^{- 1}$

Based on the above thermochemical equations, the value of $∆_{r} H °$ at 298 K for the reaction

$C_{(Graphite)} + 2 H_{2} (g) \to {CH}_{4} (g) will be :$

1. 85.2 kJ/mol

2. 15.2 kJ/mol

3. -74.8 kJ/mol

4. 74.8 kJ/mol

Subtopic: Thermochemistry |

Level 3: 35%-60%

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Q3:

In which of the following case, does the entropy decrease?

1. Boiling of egg

2. Combustion of benzene at 27^oC

3. Combustion of benzene at 127^oC

4. Dissolution of sugar in water

Subtopic: Spontaneity & Entropy |

Level 3: 35%-60%

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Q4:

At equilibrium, which of the following is always zero?

1.	$\Delta H$	2.	$\Delta S_{Total}$
3.	$\Delta S_{System}$	4.	$\Delta G^o$

Subtopic: Spontaneity & Entropy |

Level 3: 35%-60%

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Q5:

Select the correct option based on statements below:

Statement I:	Total enthalpy change of a multistep process is the sum of ∆H₁ + ∆H₂ + ∆H₃ + . . .
Statement II:	When heat is absorbed by the system, the sign of q is taken to be negative.

1.	Statement I is correct; Statement II is correct.
2.	Statement I is correct; Statement II is incorrect.
3.	Statement I is incorrect; Statement II is correct.
4.	Statement I is incorrect; Statement II is incorrect.

Subtopic: First Law of Thermodynamics |

Level 3: 35%-60%

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Q6:

At 27 ^∘C, PCl₅ is 50 % dissociated. What is the value of ∆G^o at 27 ^∘C and one atmosphere?

1. ∆G^o = -300 R ln3

2. ∆G^o = +300 R ln3

3. ∆G^o = -900 R ln3

4. ∆G^o = +900 R ln3

Subtopic: Gibbs Energy Change |

Level 3: 35%-60%

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Q7:

Based on the reactions, ascertain the valid algebraic relationship:
$(i)$ $C (g)$ $+ 4 H$ $(g)$ $\to C H_{4} (g);$
$∆ H_{r}$ $= x$ $k J$ $m o l^{- 1}$
$(i i)$ $C (g r a p h i t e)$ $+$ $2 H_{2}$ $(g)$ $\to$ $C H_{4};$
$∆ H_{r}$ $=$ $y$ $k J$ $m o l^{- 1}$

1.	x = y	2.	x = 2y
3.	x > y	4.	x < y

Subtopic: Enthalpy & Internal energy |

Level 3: 35%-60%

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Q8:

An ideal gas is expanded irreversibly against 10 bar pressure from 20 litres to 30 litres. Calculate 'w' if the process is isoenthalpic.

1.	0	2.	+100J
3.	-100 J	4.	-10 kJ

Subtopic: First Law of Thermodynamics |

Level 3: 35%-60%

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Q9:

A gas is allowed to expand in a well-insulated container against a constant external pressure of 2.5atm from an initial volume of 2.50 L to a final volume of 4.50L. The change in internal energy U of the gas in joules will be:

1.	–500J	2.	–505J
3.	–506J	4.	–508J

Subtopic: First Law of Thermodynamics |

Level 3: 35%-60%

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Q10:

Assertion (A):	The heat absorbed during the isothermal expansion of an ideal gas against a vacuum is zero.
Reason (R):	The volume occupied by the molecules of an ideal gas is zero.

1.	Both (A) and (R) are True and (R) is the correct explanation of (A).
2.	Both (A) and (R) are True but (R) is not the correct explanation of (A).
3.	(A) is True but (R) is False.
4.	(A) is False but (R) is True.

Subtopic: Enthalpy & Internal energy |

Level 3: 35%-60%

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At 27 ^∘C, PCl₅ is 50 % dissociated. What is the value of ∆G^o at 27 ^∘C and one atmosphere?

1. ∆G^o = -300 R ln3

2. ∆G^o = +300 R ln3

3. ∆G^o = -900 R ln3

4. ∆G^o = +900 R ln3

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1.	\(\Delta H\)	2.	\(\Delta S_{Total}\)
3.	\(\Delta S_{System}\)	4.	\(\Delta G^o\)

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At 27 ∘C, PCl5 is 50 % dissociated. What is the value of ∆Go at 27 ∘C and one atmosphere? 1. ∆Go = -300 R ln3 2. ∆Go = +300 R ln3 3. ∆Go = -900 R ln3 4. ∆Go = +900 R ln3

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At 27 ^∘C, PCl₅ is 50 % dissociated. What is the value of ∆G^o at 27 ^∘C and one atmosphere?

1. ∆G^o = -300 R ln3

2. ∆G^o = +300 R ln3

3. ∆G^o = -900 R ln3

4. ∆G^o = +900 R ln3