(D) In an adiabatic expansion,the system does work at the expense of its internal energy,leading to a decrease in temperature. Thus,$T_C < T_A$.For an

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(D) In an adiabatic expansion,the system does work at the expense of its internal energy,leading to a decrease in temperature. Thus,$T_C For an adiabatic process:$q = 0$,$\Delta U = W$Since it is an expansion,$W Since $\Delta U = nC_{vm} \Delta T$,we have $nC_{vm} \Delta T Therefore,$T_C - T_A Option $D$ states $T_C > T_A$,which is incorrect.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Difficult

Reversible expansion of an ideal gas under isothermal and adiabatic conditions are as shown in the figure.
$AB \to$ Isothermal expansion
$AC \to$ Adiabatic expansion
Which of the following options is not correct?

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A
$\Delta S_{\text{isothermal}} > \Delta S_{\text{adiabatic}}$
B
$T_{A} = T_{B}$
C
$W_{\text{isothermal}} > W_{\text{adiabatic}}$
D
$T_{C} > T_{A}$

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Thermodynamics

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Mix Examples-Thermodynamics and Thermochemistry

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NEET 2019 Paper All NEET years →

Match the following:

$(a)$ Entropy of vaporization $(1)$ Decreases

$(b)$ $K$ for spontaneous process $(2)$ Always has a $(+)$ value

$(c)$ Crystalline solid state $(3)$ Has minimum entropy

$(d)$ $\Delta U$ for adiabatic expansion of an ideal gas $(4)$ $\frac{\Delta H_{vap}}{T_b}$

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Identify the correct statement$(s)$:

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For the hypothetical reaction
$A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$
$\Delta_r G^o$ and $\Delta_r S^o$ are $20 \ kJ/mol$ and $-20 \ J K^{-1} mol^{-1}$ respectively at $200 \ K$.
If $\Delta_r C_P$ is $20 \ J K^{-1} mol^{-1}$ then $\Delta_r H^o$ at $400 \ K$ is.....$kJ/mol$

Medium

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What is the enthalpy of vaporization of ethanol in $kJ/mol$? Given: boiling point $(b.p.)$ = $79.5 \, ^\circ C$ and entropy change $(\Delta S_{vap})$ = $109.8 \, J K^{-1} mol^{-1}$.

Medium

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What is the difference between $\Delta H$ and $\Delta U$ for the combustion of methane at $25\,^oC$?

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$(a)$ Entropy of vaporization	$(1)$ Decreases
$(b)$ $K$ for spontaneous process	$(2)$ Always has a $(+)$ value
$(c)$ Crystalline solid state	$(3)$ Has minimum entropy
$(d)$ $\Delta U$ for adiabatic expansion of an ideal gas	$(4)$ $\frac{\Delta H_{vap}}{T_b}$

Reversible expansion of an ideal gas under isothermal and adiabatic conditions are as shown in the figure.$AB \to$ Isothermal expansion$AC \to$ Adiabatic expansionWhich of the following options is not correct?

Similar Questions

Match the following: $(a)$ Entropy of vaporization $(1)$ Decreases $(b)$ $K$ for spontaneous process $(2)$ Always has a $(+)$ value $(c)$ Crystalline solid state $(3)$ Has minimum entropy $(d)$ $\Delta U$ for adiabatic expansion of an ideal gas $(4)$ $\frac{\Delta H_{vap}}{T_b}$

Identify the correct statement$(s)$:

For the hypothetical reaction$A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$$\Delta_r G^o$ and $\Delta_r S^o$ are $20 \ kJ/mol$ and $-20 \ J K^{-1} mol^{-1}$ respectively at $200 \ K$.If $\Delta_r C_P$ is $20 \ J K^{-1} mol^{-1}$ then $\Delta_r H^o$ at $400 \ K$ is.....$kJ/mol$

What is the enthalpy of vaporization of ethanol in $kJ/mol$? Given: boiling point $(b.p.)$ = $79.5 \, ^\circ C$ and entropy change $(\Delta S_{vap})$ = $109.8 \, J K^{-1} mol^{-1}$.

What is the difference between $\Delta H$ and $\Delta U$ for the combustion of methane at $25\,^oC$?

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Reversible expansion of an ideal gas under isothermal and adiabatic conditions are as shown in the figure.
$AB \to$ Isothermal expansion
$AC \to$ Adiabatic expansion
Which of the following options is not correct?

Match the following:

$(a)$ Entropy of vaporization $(1)$ Decreases

$(b)$ $K$ for spontaneous process $(2)$ Always has a $(+)$ value

$(c)$ Crystalline solid state $(3)$ Has minimum entropy

$(d)$ $\Delta U$ for adiabatic expansion of an ideal gas $(4)$ $\frac{\Delta H_{vap}}{T_b}$

For the hypothetical reaction
$A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$
$\Delta_r G^o$ and $\Delta_r S^o$ are $20 \ kJ/mol$ and $-20 \ J K^{-1} mol^{-1}$ respectively at $200 \ K$.
If $\Delta_r C_P$ is $20 \ J K^{-1} mol^{-1}$ then $\Delta_r H^o$ at $400 \ K$ is.....$kJ/mol$