272752
What will be the entropy change of the system when expansion of $1 \mathrm{~mole}$ of a gas takes place from $3 \mathrm{~L}$ to $6 \mathrm{~L}$ under isothermal conditions? Consider, $\mathrm{R}=2 \mathrm{cal} \mathrm{K}^{-1} \mathrm{~mol}^{-1}$ and $\log 2=0.301$.
1 The standard free energy of formation of elements is zero.
2 A process that leads to increase in free energy will be spontaneous.
3 A process accompanied by decreases in entropy will be non-spontaneous under normal conditions.
4 Enthalpy of combustion is always negative.
Explanation:
$\Delta \mathrm{G}$ gives a criteria for spontaneity at constant temperature and pressure. If $\quad \Delta \mathrm{G}<0=$ Negative Then the process are spontaneous If $\Delta \mathrm{G}>0=$ Positive Then the process are non-spontaneous
J and K CET-(2011)
Thermodynamics
272757
What are the units of entropy?
1 cal.K
2 cal.K $\mathrm{K}^{-1}$
3 $\mathrm{cm} . \mathrm{K}^{-1}$
4 $\mathrm{cm} . \mathrm{K}$
Explanation:
Entropy, $\Delta \mathrm{S}=\frac{\mathrm{q}_{\mathrm{Trv}}}{\mathrm{T}}$ $\because$ unit of Entropy is cal $\mathrm{K}^{-1}$
J and K CET-(2006)
Thermodynamics
272758
One mole of a perfect gas expands isothermally to ten times its original volume. The change in entropy is
NEET Test Series from KOTA - 10 Papers In MS WORD
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Thermodynamics
272752
What will be the entropy change of the system when expansion of $1 \mathrm{~mole}$ of a gas takes place from $3 \mathrm{~L}$ to $6 \mathrm{~L}$ under isothermal conditions? Consider, $\mathrm{R}=2 \mathrm{cal} \mathrm{K}^{-1} \mathrm{~mol}^{-1}$ and $\log 2=0.301$.
1 The standard free energy of formation of elements is zero.
2 A process that leads to increase in free energy will be spontaneous.
3 A process accompanied by decreases in entropy will be non-spontaneous under normal conditions.
4 Enthalpy of combustion is always negative.
Explanation:
$\Delta \mathrm{G}$ gives a criteria for spontaneity at constant temperature and pressure. If $\quad \Delta \mathrm{G}<0=$ Negative Then the process are spontaneous If $\Delta \mathrm{G}>0=$ Positive Then the process are non-spontaneous
J and K CET-(2011)
Thermodynamics
272757
What are the units of entropy?
1 cal.K
2 cal.K $\mathrm{K}^{-1}$
3 $\mathrm{cm} . \mathrm{K}^{-1}$
4 $\mathrm{cm} . \mathrm{K}$
Explanation:
Entropy, $\Delta \mathrm{S}=\frac{\mathrm{q}_{\mathrm{Trv}}}{\mathrm{T}}$ $\because$ unit of Entropy is cal $\mathrm{K}^{-1}$
J and K CET-(2006)
Thermodynamics
272758
One mole of a perfect gas expands isothermally to ten times its original volume. The change in entropy is
272752
What will be the entropy change of the system when expansion of $1 \mathrm{~mole}$ of a gas takes place from $3 \mathrm{~L}$ to $6 \mathrm{~L}$ under isothermal conditions? Consider, $\mathrm{R}=2 \mathrm{cal} \mathrm{K}^{-1} \mathrm{~mol}^{-1}$ and $\log 2=0.301$.
1 The standard free energy of formation of elements is zero.
2 A process that leads to increase in free energy will be spontaneous.
3 A process accompanied by decreases in entropy will be non-spontaneous under normal conditions.
4 Enthalpy of combustion is always negative.
Explanation:
$\Delta \mathrm{G}$ gives a criteria for spontaneity at constant temperature and pressure. If $\quad \Delta \mathrm{G}<0=$ Negative Then the process are spontaneous If $\Delta \mathrm{G}>0=$ Positive Then the process are non-spontaneous
J and K CET-(2011)
Thermodynamics
272757
What are the units of entropy?
1 cal.K
2 cal.K $\mathrm{K}^{-1}$
3 $\mathrm{cm} . \mathrm{K}^{-1}$
4 $\mathrm{cm} . \mathrm{K}$
Explanation:
Entropy, $\Delta \mathrm{S}=\frac{\mathrm{q}_{\mathrm{Trv}}}{\mathrm{T}}$ $\because$ unit of Entropy is cal $\mathrm{K}^{-1}$
J and K CET-(2006)
Thermodynamics
272758
One mole of a perfect gas expands isothermally to ten times its original volume. The change in entropy is
272752
What will be the entropy change of the system when expansion of $1 \mathrm{~mole}$ of a gas takes place from $3 \mathrm{~L}$ to $6 \mathrm{~L}$ under isothermal conditions? Consider, $\mathrm{R}=2 \mathrm{cal} \mathrm{K}^{-1} \mathrm{~mol}^{-1}$ and $\log 2=0.301$.
1 The standard free energy of formation of elements is zero.
2 A process that leads to increase in free energy will be spontaneous.
3 A process accompanied by decreases in entropy will be non-spontaneous under normal conditions.
4 Enthalpy of combustion is always negative.
Explanation:
$\Delta \mathrm{G}$ gives a criteria for spontaneity at constant temperature and pressure. If $\quad \Delta \mathrm{G}<0=$ Negative Then the process are spontaneous If $\Delta \mathrm{G}>0=$ Positive Then the process are non-spontaneous
J and K CET-(2011)
Thermodynamics
272757
What are the units of entropy?
1 cal.K
2 cal.K $\mathrm{K}^{-1}$
3 $\mathrm{cm} . \mathrm{K}^{-1}$
4 $\mathrm{cm} . \mathrm{K}$
Explanation:
Entropy, $\Delta \mathrm{S}=\frac{\mathrm{q}_{\mathrm{Trv}}}{\mathrm{T}}$ $\because$ unit of Entropy is cal $\mathrm{K}^{-1}$
J and K CET-(2006)
Thermodynamics
272758
One mole of a perfect gas expands isothermally to ten times its original volume. The change in entropy is