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Q. No.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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At 300K, \(\Delta rG \) and \(\Delta rG^\circ \) are - 12.8 KJ mol-1 and -11.5 KJ mol-1 respectively for the following reaction:
\(A(g) + B(g) \rightleftharpoons C(l) + D(aq)\)
If the reaction is at equilibrium, then the equilibrium constant K will be:
1. \(-2.0 \times 10^0\)
2. \(1.0 \times 10^2\)
3. \(1.0 \times 10^{-2}\)
4. \(1.69 \times 10^0\)
\(A(g) + B(g) \rightleftharpoons C(l) + D(aq)\)
If the reaction is at equilibrium, then the equilibrium constant K will be:
1. \(-2.0 \times 10^0\)
2. \(1.0 \times 10^2\)
3. \(1.0 \times 10^{-2}\)
4. \(1.69 \times 10^0\)
Subtopic: Gibbs Energy Change |
Level 3: 35%-60%
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For the process
\(\mathrm{H}_2 \mathrm{O}(\mathrm{l})(1 \mathrm{bar}, 373 \mathrm{~K}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g}) (1 \mathrm{bar}, 373 \mathrm{~K})\) , the correct set of thermodynamic parameters is:
1. \( \Delta G=+\mathrm{ve}, \Delta S=0\)
2. \(\Delta G=0, \Delta S=-\mathrm{ve}\)
3. \( \Delta G=0, \Delta S=+\mathrm{ve} \)
4. \( \Delta G=-\mathrm{ve}, \Delta S=+\mathrm{ve} \)
\(\mathrm{H}_2 \mathrm{O}(\mathrm{l})(1 \mathrm{bar}, 373 \mathrm{~K}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g}) (1 \mathrm{bar}, 373 \mathrm{~K})\) , the correct set of thermodynamic parameters is:
1. \( \Delta G=+\mathrm{ve}, \Delta S=0\)
2. \(\Delta G=0, \Delta S=-\mathrm{ve}\)
3. \( \Delta G=0, \Delta S=+\mathrm{ve} \)
4. \( \Delta G=-\mathrm{ve}, \Delta S=+\mathrm{ve} \)
Subtopic: Gibbs Energy Change |
Level 3: 35%-60%
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What is the value of ∆Go at 27 ∘C and one atmosphere, if PCl5 is 50 % dissociated at 27 ∘C?
1. ∆Go = -300 R ln3
2. ∆Go = +300 R ln3
3. ∆Go = -900 R ln3
4. ∆Go = +900 R ln3
Subtopic: Gibbs Energy Change |
Level 3: 35%-60%
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Q. No.
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