272761
The enthalpy of vaporization of benzene is $+35.3 \mathrm{~kJ} / \mathrm{mol}$ at its boiling point of $80^{\circ} \mathrm{C}$. The entropy change in the transition of vapour to liquid at its boiling point is..... in $\mathrm{Jmol}^{-1} \mathrm{~K}^{-1}$
1 -100
2 +100
3 +342
4 -342
Explanation:
Given that, $\Delta \mathrm{H}_{\text {vap. }}=+35.3 \mathrm{~kJ} / \mathrm{mol}$ $\mathrm{T}=80^{\circ} \mathrm{C}=80+273=353 \mathrm{~K}$ Entropy, $\Delta \mathrm{S}_{\text {re. }}=\frac{\Delta \mathrm{H}_{\text {rzp. }}}{\mathrm{T}}=\frac{+35.3}{353}=0.1 \mathrm{~kJ} / \mathrm{mol} / \mathrm{K}$ $\Delta \mathrm{S}_{\text {vap. }}=0.1 \times 10^3=100 \mathrm{~J} / \mathrm{mol} / \mathrm{K}$ Entropy change in the transition of vapour to liquid is negative, $\Delta \mathrm{S}_{\text {vap. }}=-100 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
Karnataka-CET-2011
Thermodynamics
272749
Which of the following does not result in an increase in entropy?
1 Crystallisation of sucrose from a solution
2 Rusting of iron
3 Conversion of ice of water
4 Vaporisation of camphor
Explanation:
In crystallization of sucrose from solution, the liquid is converted into solid. As result in decrease in randomness because of which the entropy will decrease.
CG PET -2005
Thermodynamics
272750
Entropy of a perfectly crystalline solid at $0 \mathrm{~K}$ is
1 positive
2 negative
3 zero
4 either positive or negative
Explanation:
Entropy of a perfect crystalline solid at absolute zero temperature is zero. This is the statement of third law of thermodynamics.
J and K CET-(2012)
Thermodynamics
272755
When water is cooled to its entropy
1 increases
2 decreases
3 remains same
4 becomes zero
Explanation:
When water is cooled to ice randomness or disorderness decreases i.e. entropy decrease.
J and K CET-(2010)
Thermodynamics
272756
The incorrect statement among the following is
1 the entropy of the universe remains constant.
2 heat cannot be completely converted into work.
3 the absolute entropy of a perfectly crystalline solid at absolute zero temperature is zero.
4 the total energy of an isolated system remains constant.
Explanation:
The Entropy of Universe are increasing spontaneously, $\Delta \mathrm{S}_{\text {miverse }}>0$
272761
The enthalpy of vaporization of benzene is $+35.3 \mathrm{~kJ} / \mathrm{mol}$ at its boiling point of $80^{\circ} \mathrm{C}$. The entropy change in the transition of vapour to liquid at its boiling point is..... in $\mathrm{Jmol}^{-1} \mathrm{~K}^{-1}$
1 -100
2 +100
3 +342
4 -342
Explanation:
Given that, $\Delta \mathrm{H}_{\text {vap. }}=+35.3 \mathrm{~kJ} / \mathrm{mol}$ $\mathrm{T}=80^{\circ} \mathrm{C}=80+273=353 \mathrm{~K}$ Entropy, $\Delta \mathrm{S}_{\text {re. }}=\frac{\Delta \mathrm{H}_{\text {rzp. }}}{\mathrm{T}}=\frac{+35.3}{353}=0.1 \mathrm{~kJ} / \mathrm{mol} / \mathrm{K}$ $\Delta \mathrm{S}_{\text {vap. }}=0.1 \times 10^3=100 \mathrm{~J} / \mathrm{mol} / \mathrm{K}$ Entropy change in the transition of vapour to liquid is negative, $\Delta \mathrm{S}_{\text {vap. }}=-100 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
Karnataka-CET-2011
Thermodynamics
272749
Which of the following does not result in an increase in entropy?
1 Crystallisation of sucrose from a solution
2 Rusting of iron
3 Conversion of ice of water
4 Vaporisation of camphor
Explanation:
In crystallization of sucrose from solution, the liquid is converted into solid. As result in decrease in randomness because of which the entropy will decrease.
CG PET -2005
Thermodynamics
272750
Entropy of a perfectly crystalline solid at $0 \mathrm{~K}$ is
1 positive
2 negative
3 zero
4 either positive or negative
Explanation:
Entropy of a perfect crystalline solid at absolute zero temperature is zero. This is the statement of third law of thermodynamics.
J and K CET-(2012)
Thermodynamics
272755
When water is cooled to its entropy
1 increases
2 decreases
3 remains same
4 becomes zero
Explanation:
When water is cooled to ice randomness or disorderness decreases i.e. entropy decrease.
J and K CET-(2010)
Thermodynamics
272756
The incorrect statement among the following is
1 the entropy of the universe remains constant.
2 heat cannot be completely converted into work.
3 the absolute entropy of a perfectly crystalline solid at absolute zero temperature is zero.
4 the total energy of an isolated system remains constant.
Explanation:
The Entropy of Universe are increasing spontaneously, $\Delta \mathrm{S}_{\text {miverse }}>0$
272761
The enthalpy of vaporization of benzene is $+35.3 \mathrm{~kJ} / \mathrm{mol}$ at its boiling point of $80^{\circ} \mathrm{C}$. The entropy change in the transition of vapour to liquid at its boiling point is..... in $\mathrm{Jmol}^{-1} \mathrm{~K}^{-1}$
1 -100
2 +100
3 +342
4 -342
Explanation:
Given that, $\Delta \mathrm{H}_{\text {vap. }}=+35.3 \mathrm{~kJ} / \mathrm{mol}$ $\mathrm{T}=80^{\circ} \mathrm{C}=80+273=353 \mathrm{~K}$ Entropy, $\Delta \mathrm{S}_{\text {re. }}=\frac{\Delta \mathrm{H}_{\text {rzp. }}}{\mathrm{T}}=\frac{+35.3}{353}=0.1 \mathrm{~kJ} / \mathrm{mol} / \mathrm{K}$ $\Delta \mathrm{S}_{\text {vap. }}=0.1 \times 10^3=100 \mathrm{~J} / \mathrm{mol} / \mathrm{K}$ Entropy change in the transition of vapour to liquid is negative, $\Delta \mathrm{S}_{\text {vap. }}=-100 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
Karnataka-CET-2011
Thermodynamics
272749
Which of the following does not result in an increase in entropy?
1 Crystallisation of sucrose from a solution
2 Rusting of iron
3 Conversion of ice of water
4 Vaporisation of camphor
Explanation:
In crystallization of sucrose from solution, the liquid is converted into solid. As result in decrease in randomness because of which the entropy will decrease.
CG PET -2005
Thermodynamics
272750
Entropy of a perfectly crystalline solid at $0 \mathrm{~K}$ is
1 positive
2 negative
3 zero
4 either positive or negative
Explanation:
Entropy of a perfect crystalline solid at absolute zero temperature is zero. This is the statement of third law of thermodynamics.
J and K CET-(2012)
Thermodynamics
272755
When water is cooled to its entropy
1 increases
2 decreases
3 remains same
4 becomes zero
Explanation:
When water is cooled to ice randomness or disorderness decreases i.e. entropy decrease.
J and K CET-(2010)
Thermodynamics
272756
The incorrect statement among the following is
1 the entropy of the universe remains constant.
2 heat cannot be completely converted into work.
3 the absolute entropy of a perfectly crystalline solid at absolute zero temperature is zero.
4 the total energy of an isolated system remains constant.
Explanation:
The Entropy of Universe are increasing spontaneously, $\Delta \mathrm{S}_{\text {miverse }}>0$
272761
The enthalpy of vaporization of benzene is $+35.3 \mathrm{~kJ} / \mathrm{mol}$ at its boiling point of $80^{\circ} \mathrm{C}$. The entropy change in the transition of vapour to liquid at its boiling point is..... in $\mathrm{Jmol}^{-1} \mathrm{~K}^{-1}$
1 -100
2 +100
3 +342
4 -342
Explanation:
Given that, $\Delta \mathrm{H}_{\text {vap. }}=+35.3 \mathrm{~kJ} / \mathrm{mol}$ $\mathrm{T}=80^{\circ} \mathrm{C}=80+273=353 \mathrm{~K}$ Entropy, $\Delta \mathrm{S}_{\text {re. }}=\frac{\Delta \mathrm{H}_{\text {rzp. }}}{\mathrm{T}}=\frac{+35.3}{353}=0.1 \mathrm{~kJ} / \mathrm{mol} / \mathrm{K}$ $\Delta \mathrm{S}_{\text {vap. }}=0.1 \times 10^3=100 \mathrm{~J} / \mathrm{mol} / \mathrm{K}$ Entropy change in the transition of vapour to liquid is negative, $\Delta \mathrm{S}_{\text {vap. }}=-100 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
Karnataka-CET-2011
Thermodynamics
272749
Which of the following does not result in an increase in entropy?
1 Crystallisation of sucrose from a solution
2 Rusting of iron
3 Conversion of ice of water
4 Vaporisation of camphor
Explanation:
In crystallization of sucrose from solution, the liquid is converted into solid. As result in decrease in randomness because of which the entropy will decrease.
CG PET -2005
Thermodynamics
272750
Entropy of a perfectly crystalline solid at $0 \mathrm{~K}$ is
1 positive
2 negative
3 zero
4 either positive or negative
Explanation:
Entropy of a perfect crystalline solid at absolute zero temperature is zero. This is the statement of third law of thermodynamics.
J and K CET-(2012)
Thermodynamics
272755
When water is cooled to its entropy
1 increases
2 decreases
3 remains same
4 becomes zero
Explanation:
When water is cooled to ice randomness or disorderness decreases i.e. entropy decrease.
J and K CET-(2010)
Thermodynamics
272756
The incorrect statement among the following is
1 the entropy of the universe remains constant.
2 heat cannot be completely converted into work.
3 the absolute entropy of a perfectly crystalline solid at absolute zero temperature is zero.
4 the total energy of an isolated system remains constant.
Explanation:
The Entropy of Universe are increasing spontaneously, $\Delta \mathrm{S}_{\text {miverse }}>0$
272761
The enthalpy of vaporization of benzene is $+35.3 \mathrm{~kJ} / \mathrm{mol}$ at its boiling point of $80^{\circ} \mathrm{C}$. The entropy change in the transition of vapour to liquid at its boiling point is..... in $\mathrm{Jmol}^{-1} \mathrm{~K}^{-1}$
1 -100
2 +100
3 +342
4 -342
Explanation:
Given that, $\Delta \mathrm{H}_{\text {vap. }}=+35.3 \mathrm{~kJ} / \mathrm{mol}$ $\mathrm{T}=80^{\circ} \mathrm{C}=80+273=353 \mathrm{~K}$ Entropy, $\Delta \mathrm{S}_{\text {re. }}=\frac{\Delta \mathrm{H}_{\text {rzp. }}}{\mathrm{T}}=\frac{+35.3}{353}=0.1 \mathrm{~kJ} / \mathrm{mol} / \mathrm{K}$ $\Delta \mathrm{S}_{\text {vap. }}=0.1 \times 10^3=100 \mathrm{~J} / \mathrm{mol} / \mathrm{K}$ Entropy change in the transition of vapour to liquid is negative, $\Delta \mathrm{S}_{\text {vap. }}=-100 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}$
Karnataka-CET-2011
Thermodynamics
272749
Which of the following does not result in an increase in entropy?
1 Crystallisation of sucrose from a solution
2 Rusting of iron
3 Conversion of ice of water
4 Vaporisation of camphor
Explanation:
In crystallization of sucrose from solution, the liquid is converted into solid. As result in decrease in randomness because of which the entropy will decrease.
CG PET -2005
Thermodynamics
272750
Entropy of a perfectly crystalline solid at $0 \mathrm{~K}$ is
1 positive
2 negative
3 zero
4 either positive or negative
Explanation:
Entropy of a perfect crystalline solid at absolute zero temperature is zero. This is the statement of third law of thermodynamics.
J and K CET-(2012)
Thermodynamics
272755
When water is cooled to its entropy
1 increases
2 decreases
3 remains same
4 becomes zero
Explanation:
When water is cooled to ice randomness or disorderness decreases i.e. entropy decrease.
J and K CET-(2010)
Thermodynamics
272756
The incorrect statement among the following is
1 the entropy of the universe remains constant.
2 heat cannot be completely converted into work.
3 the absolute entropy of a perfectly crystalline solid at absolute zero temperature is zero.
4 the total energy of an isolated system remains constant.
Explanation:
The Entropy of Universe are increasing spontaneously, $\Delta \mathrm{S}_{\text {miverse }}>0$
