(C) According to the Gibbs equation:$\Delta G = \Delta H - T \Delta S$When $\Delta G = 0$,the system is at equilibrium,so:$\Delta H = T \Delta S$Given

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(C) According to the Gibbs equation:$\Delta G = \Delta H - T \Delta S$When $\Delta G = 0$,the system is at equilibrium,so:$\Delta H = T \Delta S$Given:$\Delta H = 40.63 \ kJ \ mol^{-1} = 40.63 \times 10^{3} \ J \ mol^{-1}$$\Delta S = 108.8 \ J \ K^{-1} \ mol^{-1}$Substituting the values:$T = \frac{\Delta H}{\Delta S}$$T = \frac{40.63 \times 10^{3} \ J \ mol^{-1}}{108.8 \ J \ K^{-1} \ mol^{-1}}$$T \approx 373.43 \ K$Thus,the temperature is approximately $373.4 \ K$.

Class 11 Chemistry Thermodynamics Free energy and Work

Medium

For vaporization of water at $1$ atmospheric pressure,the values of $\Delta H$ and $\Delta S$ are $40.63 \ kJ \ mol^{-1}$ and $108.8 \ J \ K^{-1} \ mol^{-1},$ respectively. The temperature when Gibb's energy change $(\Delta G)$ for this transformation will be zero,is ............ $K$. (in $.4$)

AIPMT 2010 All AIPMT

A
$273$
B
$393$
C
$373$
D
$293$

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Thermodynamics

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Calculate the work done during the reversible isothermal expansion of $2 \ mol$ of an ideal gas at $298 \ K$ from $10 \ L$ to $20 \ L$ in $J$. (in $.9$)

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At $273 \ K$ the maximum work done when pressure on $10 \ g$ of hydrogen is reduced from $10 \ atm$ to $1 \ atm$ under isothermal,reversible conditions is (Assume the gas behaves ideally) $(R=8.3 \ J \ K^{-1} \ mol^{-1})$

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For vaporization of water at $1$ atmospheric pressure,the values of $\Delta H$ and $\Delta S$ are $40.63 \ kJ \ mol^{-1}$ and $108.8 \ J \ K^{-1} \ mol^{-1},$ respectively. The temperature when Gibb's energy change $(\Delta G)$ for this transformation will be zero,is ............ $K$. (in $.4$)

Similar Questions

Calculate the work done during the reversible isothermal expansion of $2 \ mol$ of an ideal gas at $298 \ K$ from $10 \ L$ to $20 \ L$ in $J$. (in $.9$)

For a certain reaction,$\Delta H = -225 \ kJ \ mol^{-1}$ and $\Delta S = -150 \ J \ K^{-1} \ mol^{-1}$. Find the temperature at which $\Delta G$ is zero. (in $K$)

What is the value of $\Delta G$ for a water system in an environment with a temperature of $100 \ K$?

Calculate the maximum work done in expanding $16 \ g$ of oxygen $(O_2)$ at $300 \ K$ and occupying a volume of $5 \ dm^3$ isothermally until the volume becomes $25 \ dm^3$. (in $J$)

At $273 \ K$ the maximum work done when pressure on $10 \ g$ of hydrogen is reduced from $10 \ atm$ to $1 \ atm$ under isothermal,reversible conditions is (Assume the gas behaves ideally) $(R=8.3 \ J \ K^{-1} \ mol^{-1})$

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