(C) The work done in an expansion process is given by the formula $W = -P_{ext} \times \Delta V$.Since the gas is expanding into a vacuum bulb,the ext

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(C) The work done in an expansion process is given by the formula $W = -P_{ext} \times \Delta V$.Since the gas is expanding into a vacuum bulb,the external pressure $P_{ext}$ is equal to $0 \ atm$.Therefore,$W = -0 \times \Delta V = 0 \ J$.

Class 11 Chemistry Thermodynamics Free energy and Work

Easy

One mole of an ideal gas at $1 \ atm$ pressure is filled in a bulb of $10 \ L$ capacity and is connected to a vacuum bulb of $100 \ L$ capacity. How much work is done in this process in Joules?

A
$405.3$
B
$203.3$
C
$0$
D
$63.3$

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Class 11

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Thermodynamics

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Free energy and Work

If an endothermic reaction is non-spontaneous at the freezing point of water and becomes feasible at its boiling point,then:

MediumAIEEE 2002

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For a reaction to occur spontaneously,which of the following conditions must be met?

MediumAIPMT 1995

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For water,the value of $\Delta H_{vap}$ is $40.73 \, kJ \, mol^{-1}$ and the value of $\Delta S_{vap}$ is $109 \, J \, K^{-1} \, mol^{-1}$. At what temperature will water be in equilibrium with its vapor?

Difficult

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If the enthalpy and entropy change for a reaction at $298 \ K$ are $-145 \ kJ \ mol^{-1}$ and $-650 \ J \ K^{-1} \ mol^{-1}$ respectively,which one of the following statements is correct?

EasyAP EAMCET 2023

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For the reaction $PCl_5 \to PCl_3 + Cl_2$,$\Delta H = 75 \ kJ \ mol^{-1}$ and $\Delta S = 120 \ J \ K^{-1} \ mol^{-1}$. At which temperature will the reaction be spontaneous? (in $K$)

Medium

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One mole of an ideal gas at $1 \ atm$ pressure is filled in a bulb of $10 \ L$ capacity and is connected to a vacuum bulb of $100 \ L$ capacity. How much work is done in this process in Joules?

Similar Questions

If an endothermic reaction is non-spontaneous at the freezing point of water and becomes feasible at its boiling point,then:

For a reaction to occur spontaneously,which of the following conditions must be met?

For water,the value of $\Delta H_{vap}$ is $40.73 \, kJ \, mol^{-1}$ and the value of $\Delta S_{vap}$ is $109 \, J \, K^{-1} \, mol^{-1}$. At what temperature will water be in equilibrium with its vapor?

If the enthalpy and entropy change for a reaction at $298 \ K$ are $-145 \ kJ \ mol^{-1}$ and $-650 \ J \ K^{-1} \ mol^{-1}$ respectively,which one of the following statements is correct?

For the reaction $PCl_5 \to PCl_3 + Cl_2$,$\Delta H = 75 \ kJ \ mol^{-1}$ and $\Delta S = 120 \ J \ K^{-1} \ mol^{-1}$. At which temperature will the reaction be spontaneous? (in $K$)

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