(B) For an ideal gas,the change in internal energy is given by $\Delta U = n \times C_v \times \Delta T$. Given $n = 5 \, mol$,$C_v = 28 \, J \, K^{-1

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$\Delta U = 14 \, kJ ; \Delta (pV) = 4 \, kJ$

(B) For an ideal gas,the change in internal energy is given by $\Delta U = n \times C_v \times \Delta T$. Given $n = 5 \, mol$,$C_v = 28 \, J \, K^{-1} \, mol^{-1}$,and $\Delta T = 200 \, K - 100 \, K = 100 \, K$. $\Delta U = 5 \times 28 \times 100 = 14000 \, J = 14 \, kJ$. For an ideal gas,$\Delta (pV) = nR\Delta T$. Given $R = 8.0 \, J \, K^{-1} \, mol^{-1}$. $\Delta (pV) = 5 \times 8 \times 100 = 4000 \, J = 4 \, kJ$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Difficult

$5 \, mol$ of an ideal gas at $100 \, K$ are allowed to undergo reversible compression till its temperature becomes $200 \, K$. If $C_v = 28 \, J \, K^{-1} \, mol^{-1}$,calculate $\Delta U$ and $\Delta pV$ for this process. $(R = 8.0 \, J \, K^{-1} \, mol^{-1})$

JEE MAIN 2019 All JEE MAIN

A
$\Delta U = 2.8 \, kJ ; \Delta (pV) = 0.8 \, kJ$
B
$\Delta U = 14 \, kJ ; \Delta (pV) = 4 \, kJ$
C
$\Delta U = 14 \, kJ ; \Delta (pV) = 18 \, kJ$
D
$\Delta U = 14 \, kJ ; \Delta (pV) = 0.8 \, J$

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Two moles of an ideal monoatomic gas are allowed to expand adiabatically and reversibly from $300 \ K$ to $200 \ K$. The work done in the process will be $..... \ kJ$.

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For the reaction: $A_{(g)} + B_{(s)} \rightleftharpoons 2C_{(g)} + D_{(g)}$,given $\Delta U = 5.0 \ kcal$ and $\Delta S = 50 \ cal \ K^{-1}$ at $400 \ K$. Calculate $\Delta G$ for the reaction. (in $kcal$)

Medium

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For an isothermal expansion of $2 \, \text{mol}$ of a gas at $298 \, K$ from $5 \, dm^3$ to $40 \, dm^3$ under constant external pressure,the work done $(W)$ and the reversible work $(W_{rev})$ are,respectively:

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The enthalpy of neutralisation of $KOH$ by a weak acid $(HA)$ is $-12.2 \ kcal \ mol^{-1}$. If the weak acid is $10 \%$ ionised,then the enthalpy of dissociation of $1 \ mole$ of $HA$ is. Given that the enthalpy of neutralisation of $KOH$ by $HCl$ is $-13.7 \ kcal \ mol^{-1}$.

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Enthalpy of neutralisation of acetic acid by $NaOH$ is $-50.6 \ kJ/mol$ and the heat of neutralisation of a strong acid with a strong base is $-55.9 \ kJ/mol$. What is the value of $\Delta H$ for the ionisation of $CH_3COOH$ in $kJ/mol$?

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$5 \, mol$ of an ideal gas at $100 \, K$ are allowed to undergo reversible compression till its temperature becomes $200 \, K$. If $C_v = 28 \, J \, K^{-1} \, mol^{-1}$,calculate $\Delta U$ and $\Delta pV$ for this process. $(R = 8.0 \, J \, K^{-1} \, mol^{-1})$

Similar Questions

Two moles of an ideal monoatomic gas are allowed to expand adiabatically and reversibly from $300 \ K$ to $200 \ K$. The work done in the process will be $..... \ kJ$.

For the reaction: $A_{(g)} + B_{(s)} \rightleftharpoons 2C_{(g)} + D_{(g)}$,given $\Delta U = 5.0 \ kcal$ and $\Delta S = 50 \ cal \ K^{-1}$ at $400 \ K$. Calculate $\Delta G$ for the reaction. (in $kcal$)

For an isothermal expansion of $2 \, \text{mol}$ of a gas at $298 \, K$ from $5 \, dm^3$ to $40 \, dm^3$ under constant external pressure,the work done $(W)$ and the reversible work $(W_{rev})$ are,respectively:

The enthalpy of neutralisation of $KOH$ by a weak acid $(HA)$ is $-12.2 \ kcal \ mol^{-1}$. If the weak acid is $10 \%$ ionised,then the enthalpy of dissociation of $1 \ mole$ of $HA$ is. Given that the enthalpy of neutralisation of $KOH$ by $HCl$ is $-13.7 \ kcal \ mol^{-1}$.

Enthalpy of neutralisation of acetic acid by $NaOH$ is $-50.6 \ kJ/mol$ and the heat of neutralisation of a strong acid with a strong base is $-55.9 \ kJ/mol$. What is the value of $\Delta H$ for the ionisation of $CH_3COOH$ in $kJ/mol$?

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