Absolute Entropy and Third Law of Thermodynamics
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CHXI06:THERMODYNAMICS

369291 Which of the following statement is false regarding entropy?

1 The greater the disorder in an isolated system, the lower is the entropy.
2 The entropy change can be attributed to rearrangement of atoms or ions from one pattern in the reactants to another (in the product).
3 Decrease of regularity in structure would mean increase in entropy.
4 The gaseous state is the state of highest entropy.
CHXI06:THERMODYNAMICS

369292 The entropy change can be calculated by using the expression \(\mathrm{\Delta S=\dfrac{q_{r e v}}{T}}\). When water freezes in a glass beaker, choose the correct statement amongst the following:

1 \(\mathrm{\Delta S}\) (system) decrease bu \(\mathrm{\Delta S}\) (surroundings remains the same
2 \(\mathrm{\Delta S}\) (system) increases but \(\mathrm{\Delta S}\) (surroundings) decreases.
3 \(\mathrm{\Delta S}\) (system) decreases but \(\mathrm{\Delta S}\) (surroundings) increases.
4 \(\mathrm{\Delta S}\) (system) decreases and \(\mathrm{\Delta S}\) (surroundings) both decreases.
NCERT Exemplar
CHXI06:THERMODYNAMICS

369293 Calculate \(\mathrm{\Delta_{\mathrm{r}} \mathrm{S}_{\mathrm{sys}}^{o}}\) for the following reaction at 373 \(\mathrm{\mathrm{KCO}_{(\mathrm{g})}+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})}}\)
\(\mathrm{\Delta_{\mathrm{r}} \mathrm{H}^{\circ}=-4.1 \times 10^{4} \mathrm{~J}, \Delta_{\mathrm{r}} \mathrm{S}_{\text {univ }}^{o}=56 \mathrm{~J} / \mathrm{K}}\)

1 \(\mathrm{-54 \mathrm{~J} / \mathrm{K}}\)
2 \(\mathrm{-166 \mathrm{~J} / \mathrm{K}}\)
3 \(\mathrm{+54 \mathrm{~J} / \mathrm{K}}\)
4 \(\mathrm{+166 \mathrm{~J} / \mathrm{Ks}}\)
CHXI06:THERMODYNAMICS

369294 Calculate the entropy change in surroundings when \(\mathrm{1.00 \mathrm{~mol}}\) of \(\mathrm{\mathrm{H}_{2} \mathrm{O}(\mathrm{l})}\) is formed under standard conditions. \(\mathrm{\Delta_{\mathrm{f}} \mathrm{H}^{\circ}=-286 \mathrm{~kJ} \mathrm{~mol}^{-1}}\).

1 \({\rm{960}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
2 \({\rm{960}}\,{\rm{k}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
3 \({\rm{1048}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
4 \({\rm{1048}}\,{\rm{k}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
CHXI06:THERMODYNAMICS

369295 For a process, entropy change of a system is expressed as

1 \(\mathrm{\mathrm{H}-\mathrm{TS}}\)
2 \(\mathrm{\dfrac{q_{\text {rev }}}{T}}\)
3 \(\mathrm{\dfrac{\mathrm{T}}{\mathrm{q}_{\mathrm{rev}}}}\)
4 \(\mathrm{q_{\text {rev }} \times T}\)
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CHXI06:THERMODYNAMICS

369291 Which of the following statement is false regarding entropy?

1 The greater the disorder in an isolated system, the lower is the entropy.
2 The entropy change can be attributed to rearrangement of atoms or ions from one pattern in the reactants to another (in the product).
3 Decrease of regularity in structure would mean increase in entropy.
4 The gaseous state is the state of highest entropy.
CHXI06:THERMODYNAMICS

369292 The entropy change can be calculated by using the expression \(\mathrm{\Delta S=\dfrac{q_{r e v}}{T}}\). When water freezes in a glass beaker, choose the correct statement amongst the following:

1 \(\mathrm{\Delta S}\) (system) decrease bu \(\mathrm{\Delta S}\) (surroundings remains the same
2 \(\mathrm{\Delta S}\) (system) increases but \(\mathrm{\Delta S}\) (surroundings) decreases.
3 \(\mathrm{\Delta S}\) (system) decreases but \(\mathrm{\Delta S}\) (surroundings) increases.
4 \(\mathrm{\Delta S}\) (system) decreases and \(\mathrm{\Delta S}\) (surroundings) both decreases.
NCERT Exemplar
CHXI06:THERMODYNAMICS

369293 Calculate \(\mathrm{\Delta_{\mathrm{r}} \mathrm{S}_{\mathrm{sys}}^{o}}\) for the following reaction at 373 \(\mathrm{\mathrm{KCO}_{(\mathrm{g})}+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})}}\)
\(\mathrm{\Delta_{\mathrm{r}} \mathrm{H}^{\circ}=-4.1 \times 10^{4} \mathrm{~J}, \Delta_{\mathrm{r}} \mathrm{S}_{\text {univ }}^{o}=56 \mathrm{~J} / \mathrm{K}}\)

1 \(\mathrm{-54 \mathrm{~J} / \mathrm{K}}\)
2 \(\mathrm{-166 \mathrm{~J} / \mathrm{K}}\)
3 \(\mathrm{+54 \mathrm{~J} / \mathrm{K}}\)
4 \(\mathrm{+166 \mathrm{~J} / \mathrm{Ks}}\)
CHXI06:THERMODYNAMICS

369294 Calculate the entropy change in surroundings when \(\mathrm{1.00 \mathrm{~mol}}\) of \(\mathrm{\mathrm{H}_{2} \mathrm{O}(\mathrm{l})}\) is formed under standard conditions. \(\mathrm{\Delta_{\mathrm{f}} \mathrm{H}^{\circ}=-286 \mathrm{~kJ} \mathrm{~mol}^{-1}}\).

1 \({\rm{960}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
2 \({\rm{960}}\,{\rm{k}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
3 \({\rm{1048}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
4 \({\rm{1048}}\,{\rm{k}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
CHXI06:THERMODYNAMICS

369295 For a process, entropy change of a system is expressed as

1 \(\mathrm{\mathrm{H}-\mathrm{TS}}\)
2 \(\mathrm{\dfrac{q_{\text {rev }}}{T}}\)
3 \(\mathrm{\dfrac{\mathrm{T}}{\mathrm{q}_{\mathrm{rev}}}}\)
4 \(\mathrm{q_{\text {rev }} \times T}\)
MHTCET - 2019
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CHXI06:THERMODYNAMICS

369291 Which of the following statement is false regarding entropy?

1 The greater the disorder in an isolated system, the lower is the entropy.
2 The entropy change can be attributed to rearrangement of atoms or ions from one pattern in the reactants to another (in the product).
3 Decrease of regularity in structure would mean increase in entropy.
4 The gaseous state is the state of highest entropy.
CHXI06:THERMODYNAMICS

369292 The entropy change can be calculated by using the expression \(\mathrm{\Delta S=\dfrac{q_{r e v}}{T}}\). When water freezes in a glass beaker, choose the correct statement amongst the following:

1 \(\mathrm{\Delta S}\) (system) decrease bu \(\mathrm{\Delta S}\) (surroundings remains the same
2 \(\mathrm{\Delta S}\) (system) increases but \(\mathrm{\Delta S}\) (surroundings) decreases.
3 \(\mathrm{\Delta S}\) (system) decreases but \(\mathrm{\Delta S}\) (surroundings) increases.
4 \(\mathrm{\Delta S}\) (system) decreases and \(\mathrm{\Delta S}\) (surroundings) both decreases.
NCERT Exemplar
CHXI06:THERMODYNAMICS

369293 Calculate \(\mathrm{\Delta_{\mathrm{r}} \mathrm{S}_{\mathrm{sys}}^{o}}\) for the following reaction at 373 \(\mathrm{\mathrm{KCO}_{(\mathrm{g})}+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})}}\)
\(\mathrm{\Delta_{\mathrm{r}} \mathrm{H}^{\circ}=-4.1 \times 10^{4} \mathrm{~J}, \Delta_{\mathrm{r}} \mathrm{S}_{\text {univ }}^{o}=56 \mathrm{~J} / \mathrm{K}}\)

1 \(\mathrm{-54 \mathrm{~J} / \mathrm{K}}\)
2 \(\mathrm{-166 \mathrm{~J} / \mathrm{K}}\)
3 \(\mathrm{+54 \mathrm{~J} / \mathrm{K}}\)
4 \(\mathrm{+166 \mathrm{~J} / \mathrm{Ks}}\)
CHXI06:THERMODYNAMICS

369294 Calculate the entropy change in surroundings when \(\mathrm{1.00 \mathrm{~mol}}\) of \(\mathrm{\mathrm{H}_{2} \mathrm{O}(\mathrm{l})}\) is formed under standard conditions. \(\mathrm{\Delta_{\mathrm{f}} \mathrm{H}^{\circ}=-286 \mathrm{~kJ} \mathrm{~mol}^{-1}}\).

1 \({\rm{960}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
2 \({\rm{960}}\,{\rm{k}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
3 \({\rm{1048}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
4 \({\rm{1048}}\,{\rm{k}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
CHXI06:THERMODYNAMICS

369295 For a process, entropy change of a system is expressed as

1 \(\mathrm{\mathrm{H}-\mathrm{TS}}\)
2 \(\mathrm{\dfrac{q_{\text {rev }}}{T}}\)
3 \(\mathrm{\dfrac{\mathrm{T}}{\mathrm{q}_{\mathrm{rev}}}}\)
4 \(\mathrm{q_{\text {rev }} \times T}\)
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CHXI06:THERMODYNAMICS

369291 Which of the following statement is false regarding entropy?

1 The greater the disorder in an isolated system, the lower is the entropy.
2 The entropy change can be attributed to rearrangement of atoms or ions from one pattern in the reactants to another (in the product).
3 Decrease of regularity in structure would mean increase in entropy.
4 The gaseous state is the state of highest entropy.
CHXI06:THERMODYNAMICS

369292 The entropy change can be calculated by using the expression \(\mathrm{\Delta S=\dfrac{q_{r e v}}{T}}\). When water freezes in a glass beaker, choose the correct statement amongst the following:

1 \(\mathrm{\Delta S}\) (system) decrease bu \(\mathrm{\Delta S}\) (surroundings remains the same
2 \(\mathrm{\Delta S}\) (system) increases but \(\mathrm{\Delta S}\) (surroundings) decreases.
3 \(\mathrm{\Delta S}\) (system) decreases but \(\mathrm{\Delta S}\) (surroundings) increases.
4 \(\mathrm{\Delta S}\) (system) decreases and \(\mathrm{\Delta S}\) (surroundings) both decreases.
NCERT Exemplar
CHXI06:THERMODYNAMICS

369293 Calculate \(\mathrm{\Delta_{\mathrm{r}} \mathrm{S}_{\mathrm{sys}}^{o}}\) for the following reaction at 373 \(\mathrm{\mathrm{KCO}_{(\mathrm{g})}+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})}}\)
\(\mathrm{\Delta_{\mathrm{r}} \mathrm{H}^{\circ}=-4.1 \times 10^{4} \mathrm{~J}, \Delta_{\mathrm{r}} \mathrm{S}_{\text {univ }}^{o}=56 \mathrm{~J} / \mathrm{K}}\)

1 \(\mathrm{-54 \mathrm{~J} / \mathrm{K}}\)
2 \(\mathrm{-166 \mathrm{~J} / \mathrm{K}}\)
3 \(\mathrm{+54 \mathrm{~J} / \mathrm{K}}\)
4 \(\mathrm{+166 \mathrm{~J} / \mathrm{Ks}}\)
CHXI06:THERMODYNAMICS

369294 Calculate the entropy change in surroundings when \(\mathrm{1.00 \mathrm{~mol}}\) of \(\mathrm{\mathrm{H}_{2} \mathrm{O}(\mathrm{l})}\) is formed under standard conditions. \(\mathrm{\Delta_{\mathrm{f}} \mathrm{H}^{\circ}=-286 \mathrm{~kJ} \mathrm{~mol}^{-1}}\).

1 \({\rm{960}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
2 \({\rm{960}}\,{\rm{k}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
3 \({\rm{1048}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
4 \({\rm{1048}}\,{\rm{k}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
CHXI06:THERMODYNAMICS

369295 For a process, entropy change of a system is expressed as

1 \(\mathrm{\mathrm{H}-\mathrm{TS}}\)
2 \(\mathrm{\dfrac{q_{\text {rev }}}{T}}\)
3 \(\mathrm{\dfrac{\mathrm{T}}{\mathrm{q}_{\mathrm{rev}}}}\)
4 \(\mathrm{q_{\text {rev }} \times T}\)
MHTCET - 2019
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CHXI06:THERMODYNAMICS

369291 Which of the following statement is false regarding entropy?

1 The greater the disorder in an isolated system, the lower is the entropy.
2 The entropy change can be attributed to rearrangement of atoms or ions from one pattern in the reactants to another (in the product).
3 Decrease of regularity in structure would mean increase in entropy.
4 The gaseous state is the state of highest entropy.
CHXI06:THERMODYNAMICS

369292 The entropy change can be calculated by using the expression \(\mathrm{\Delta S=\dfrac{q_{r e v}}{T}}\). When water freezes in a glass beaker, choose the correct statement amongst the following:

1 \(\mathrm{\Delta S}\) (system) decrease bu \(\mathrm{\Delta S}\) (surroundings remains the same
2 \(\mathrm{\Delta S}\) (system) increases but \(\mathrm{\Delta S}\) (surroundings) decreases.
3 \(\mathrm{\Delta S}\) (system) decreases but \(\mathrm{\Delta S}\) (surroundings) increases.
4 \(\mathrm{\Delta S}\) (system) decreases and \(\mathrm{\Delta S}\) (surroundings) both decreases.
NCERT Exemplar
CHXI06:THERMODYNAMICS

369293 Calculate \(\mathrm{\Delta_{\mathrm{r}} \mathrm{S}_{\mathrm{sys}}^{o}}\) for the following reaction at 373 \(\mathrm{\mathrm{KCO}_{(\mathrm{g})}+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})} \rightarrow \mathrm{CO}_{2(\mathrm{~g})}+\mathrm{H}_{2(\mathrm{~g})}}\)
\(\mathrm{\Delta_{\mathrm{r}} \mathrm{H}^{\circ}=-4.1 \times 10^{4} \mathrm{~J}, \Delta_{\mathrm{r}} \mathrm{S}_{\text {univ }}^{o}=56 \mathrm{~J} / \mathrm{K}}\)

1 \(\mathrm{-54 \mathrm{~J} / \mathrm{K}}\)
2 \(\mathrm{-166 \mathrm{~J} / \mathrm{K}}\)
3 \(\mathrm{+54 \mathrm{~J} / \mathrm{K}}\)
4 \(\mathrm{+166 \mathrm{~J} / \mathrm{Ks}}\)
CHXI06:THERMODYNAMICS

369294 Calculate the entropy change in surroundings when \(\mathrm{1.00 \mathrm{~mol}}\) of \(\mathrm{\mathrm{H}_{2} \mathrm{O}(\mathrm{l})}\) is formed under standard conditions. \(\mathrm{\Delta_{\mathrm{f}} \mathrm{H}^{\circ}=-286 \mathrm{~kJ} \mathrm{~mol}^{-1}}\).

1 \({\rm{960}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
2 \({\rm{960}}\,{\rm{k}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
3 \({\rm{1048}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
4 \({\rm{1048}}\,{\rm{k}}\,{\rm{J}}\,{{\rm{K}}^{{\rm{ - 1}}}}{\rm{\;mo}}{{\rm{l}}^{{\rm{ - 1}}}}\)
CHXI06:THERMODYNAMICS

369295 For a process, entropy change of a system is expressed as

1 \(\mathrm{\mathrm{H}-\mathrm{TS}}\)
2 \(\mathrm{\dfrac{q_{\text {rev }}}{T}}\)
3 \(\mathrm{\dfrac{\mathrm{T}}{\mathrm{q}_{\mathrm{rev}}}}\)
4 \(\mathrm{q_{\text {rev }} \times T}\)
MHTCET - 2019