(A) Step $1$: Calculate $\Delta_r H^o$ at $200 \ K$ using the relation $\Delta G^o = \Delta H^o - T \Delta S^o$.$\Delta H_{200}^o = \Delta G_{200}^o +

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(A) Step $1$: Calculate $\Delta_r H^o$ at $200 \ K$ using the relation $\Delta G^o = \Delta H^o - T \Delta S^o$.$\Delta H_{200}^o = \Delta G_{200}^o + T \Delta S_{200}^o = 20 \ kJ/mol + (200 \ K \times (-20 \ J K^{-1} mol^{-1})) / 1000 = 20 - 4 = 16 \ kJ/mol$.Step $2$: Calculate $\Delta_r H^o$ at $400 \ K$ using Kirchhoff's equation: $\Delta H_{T_2}^o = \Delta H_{T_1}^o + \Delta_r C_P (T_2 - T_1)$.$\Delta H_{400}^o = 16 \ kJ/mol + (20 \ J K^{-1} mol^{-1} \times (400 \ K - 200 \ K)) / 1000$.$\Delta H_{400}^o = 16 + (20 \times 200) / 1000 = 16 + 4 = 20 \ kJ/mol$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

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.....$kJ/mol$

A
$20$
B
$7.98$
C
$28$
D
None of these

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MediumTS EAMCET 2024

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$20.0 \ dm^{3}$ of an ideal gas '$X$' at $600 \ K$ and $0.5 \ MPa$ undergoes isothermal reversible expansion until the pressure of the gas is $0.2 \ MPa$. Which of the following options is correct? (Given: $\log\,2=0.3010$ and $\log\,5=0.6989$)

DifficultJEE MAIN 2026

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The amount of heat released when $20 \ mL$ of $0.5 \ M$ $NaOH$ is mixed with $100 \ mL$ of $0.1 \ M$ $HCl$ is $x \ kJ$. The heat of neutralization is:

EasyWBJEE 2011

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The value of $\Delta H_{transition}$ for $C(\text{graphite}) \rightarrow C(\text{diamond})$ is $1.9 \ kJ/mol$ at $25^{\circ}C$. The entropy of graphite is higher than the entropy of diamond. This implies that which of the following is incorrect $:-$

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$A$ solution of $500 \ mL$ of $0.2 \ M \ KOH$ and $500 \ mL$ of $0.2 \ M \ HCl$ is mixed and stirred; the rise in temperature is $T_1$. The experiment is repeated using $250 \ mL$ each of solution,the temperature raised is $T_2$. Which of the following is true?

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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.....$kJ/mol$

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$20.0 \ dm^{3}$ of an ideal gas '$X$' at $600 \ K$ and $0.5 \ MPa$ undergoes isothermal reversible expansion until the pressure of the gas is $0.2 \ MPa$. Which of the following options is correct? (Given: $\log\,2=0.3010$ and $\log\,5=0.6989$)

The amount of heat released when $20 \ mL$ of $0.5 \ M$ $NaOH$ is mixed with $100 \ mL$ of $0.1 \ M$ $HCl$ is $x \ kJ$. The heat of neutralization is:

The value of $\Delta H_{transition}$ for $C(\text{graphite}) \rightarrow C(\text{diamond})$ is $1.9 \ kJ/mol$ at $25^{\circ}C$. The entropy of graphite is higher than the entropy of diamond. This implies that which of the following is incorrect $:-$

$A$ solution of $500 \ mL$ of $0.2 \ M \ KOH$ and $500 \ mL$ of $0.2 \ M \ HCl$ is mixed and stirred; the rise in temperature is $T_1$. The experiment is repeated using $250 \ mL$ each of solution,the temperature raised is $T_2$. Which of the following is true?

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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.....$kJ/mol$