(B) At the boiling point,the process of vaporization is in equilibrium,so $\Delta G = 0$. Using the relation $\Delta G = \Delta H - T\Delta S$,we get

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(B) At the boiling point,the process of vaporization is in equilibrium,so $\Delta G = 0$. Using the relation $\Delta G = \Delta H - T\Delta S$,we get $\Delta H = T\Delta S$. Given $\Delta H = 30 \ kJ \ mol^{-1} = 30000 \ J \ mol^{-1}$ and $\Delta S = 75 \ J \ mol^{-1} \ K^{-1}$. $T = \frac{\Delta H}{\Delta S} = \frac{30000 \ J \ mol^{-1}}{75 \ J \ mol^{-1} \ K^{-1}} = 400 \ K$.

Class 11 Chemistry Thermodynamics 2 nd Law of thermodynamics and Entropy

Medium

The enthalpy of vapourization of a liquid is $30 \ kJ \ mol^{-1}$ and entropy of vapourization is $75 \ J \ mol^{-1} \ K^{-1}$. The boiling point of the liquid at $1 \ atm$ is.......$K$

IIT 2004 All IIT

A
$250$
B
$400$
C
$450$
D
$600$

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Class 11 Questions

Class 11

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Chapter

Thermodynamics

Subtopic

2 nd Law of thermodynamics and Entropy

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IIT 2004 Paper All IIT years →

One mole of which of the following has the highest entropy?

MediumKCET 2008

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At $10\, ^oC$,$1\, mol$ of an ideal gas is allowed to expand reversibly and adiabatically from $10\, L$ to $200\, L$. Calculate the change in entropy in $cal/K$.

Easy

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One mole of water at $100\,^{\circ}C$ is converted into steam at $100\,^{\circ}C$ at a constant pressure of $1\,atm$. The change in entropy is [heat of vaporisation of water at $100\,^{\circ}C = 540\,cal/g$].

Medium

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Given that $\Delta H = 0$ for the mixing of two gases,explain whether the diffusion of these gases into each other in a closed container is a spontaneous process or not?

Easy

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$A$ container has a hydrogen and oxygen mixture in a ratio of $4 : 1$ by weight. When these gases are mixed,which of the following occurs?

Easy

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The enthalpy of vapourization of a liquid is $30 \ kJ \ mol^{-1}$ and entropy of vapourization is $75 \ J \ mol^{-1} \ K^{-1}$. The boiling point of the liquid at $1 \ atm$ is.......$K$

Similar Questions

One mole of which of the following has the highest entropy?

At $10\, ^oC$,$1\, mol$ of an ideal gas is allowed to expand reversibly and adiabatically from $10\, L$ to $200\, L$. Calculate the change in entropy in $cal/K$.

One mole of water at $100\,^{\circ}C$ is converted into steam at $100\,^{\circ}C$ at a constant pressure of $1\,atm$. The change in entropy is [heat of vaporisation of water at $100\,^{\circ}C = 540\,cal/g$].

Given that $\Delta H = 0$ for the mixing of two gases,explain whether the diffusion of these gases into each other in a closed container is a spontaneous process or not?

$A$ container has a hydrogen and oxygen mixture in a ratio of $4 : 1$ by weight. When these gases are mixed,which of the following occurs?

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