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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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 |
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,
$$\mathrm{Ag_2 CO_3 (s) \rightarrow 2Ag^+ (aq) + CO^{2-}_3 (aq)}$$
$$\mathrm{K_{sp}}$$ 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. $$7.9 \times 10^{-2}$$
Subtopic:  Gibbs Energy Change |
60%
From NCERT
AIPMT - 2014
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Given the reaction:
X2O4(l) → 2XO2(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 ($$\Delta$$Hcomb. (CH4) = 890 kJ mol–1, $$\Delta$$Hcomb( C3H8) = 2220 kJ mol–1) is:
1. 38
2. 317
3. 477
4. 32
Subtopic:  Thermochemistry |
61%
From NCERT
NEET - 2013
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Three thermochemical equations are given below:
 (i) C(graphite) + O2(g) $$\rightarrow$$ CO2(g); $$\Delta_{r}$$H° = x kJ mol–1 (ii) Cgraphite + 1/2 O2(g) $$\rightarrow$$ CO(g); $$\Delta_{r}$$H° = y kJ mol–1 (iii) CO(g) + 1/2 O2(g) $$\rightarrow$$ CO2(g); $$\Delta_{r}$$H° = z kJ mol–1

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

In which of the following reactions, the standard reaction entropy change
$\left(∆{S}^{0}\right)$ is positive, and standard Gibb's energy change
$\left(∆{G}^{0}\right)$ decreases sharply with increasing temperature?

 1 C(graphite) + $$\frac{1}{2}$$O2(g) → CO(g) 2 CO(g) + $$\frac{1}{2}$$O2(g) → CO2(g) 3 Mg(s) + $$\frac{1}{2}$$O2(g) → MgO(s) 4 $$\frac{1}{2}$$C(graphite) + $$\frac{1}{2}$$O2(g) → $$\frac{1}{2}$$CO2(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 oC 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 ${∆}_{\mathrm{vap}}{\mathrm{H}}^{o}$ for water at 100 oC is 40.66 kJ mol-1.
The internal energy of vaporization of water at 100 oC (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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Equal volumes of two monoatomic gases, A and B, at same temperature and pressure are mixed. The ratio of specific heats (Cp/Cv) of the mixture will be:
1.  1.50
2.  3.3
3.  1.67
4.  0.83

Subtopic:  Cp & Cv |
78%
AIPMT - 2012
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