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

Subtopic:  2nd & 3rd Law of Thermodynamics |
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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

Subtopic:  Gibbs Energy Change |
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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. H2(g)+Br2(g)2HBr(g)

2. C(s)+2H2O(g)2H2(g)+CO2(g)

3. PCl5(g)PCl3(g)+Cl2(g)

4. 2COg+O2g2CO2g

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 fG0 of the sulphide is greater than those for CS2 and H2S

3. The fG0 is negative for roasting of sulphur ore to oxide.

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

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 ΔHf for HCl is -90 kJ mol-1. The bond enthalpy of HCl is :

1. 290 kJ mol-1

2. 380 kJ mol-1

3. 425 kJ mol-1

4. 245 kJ mol-1

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

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 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 |
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For the gas phase reaction, 
 PCl5(g)PCl3(g)+Cl2(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

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

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

Subtopic:  Thermochemistry |
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