(A) The reaction is $3 A_{(g)} \rightarrow 2 B_{(g)} + 2 D_{(g)} + E_{(g)}$.The change in moles of gaseous products is $\Delta n_g = (2 + 2 + 1) - 3 =

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Reaction is spontaneous and $\Delta G = -1.2 \ kcal / mol$

(A) The reaction is $3 A_{(g)} \rightarrow 2 B_{(g)} + 2 D_{(g)} + E_{(g)}$.The change in moles of gaseous products is $\Delta n_g = (2 + 2 + 1) - 3 = 2$.Given $\Delta U = 5.1 \ kcal / mol$,$\Delta S = 25 \ cal / mol \cdot K = 0.025 \ kcal / mol \cdot K$,and $T = 300 \ K$.Calculate $\Delta H$ using $\Delta H = \Delta U + \Delta n_g RT$:$\Delta H = 5.1 + \frac{2 \times 2 \times 300}{1000} = 5.1 + 1.2 = 6.3 \ kcal / mol$.Calculate $\Delta G$ using $\Delta G = \Delta H - T \Delta S$:$\Delta G = 6.3 - (300 \times 0.025) = 6.3 - 7.5 = -1.2 \ kcal / mol$.Since $\Delta G < 0$,the reaction is spontaneous.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

$3 A_{(g)} \rightarrow 2 B_{(g)} + 2 D_{(g)} + E_{(g)}$
For the above reaction,$\Delta U = 5.1 \ kcal / mol$ and $\Delta S = 25 \ cal / mol \cdot K$. Which of the following is the correct statement at $300 \ K$?

A
Reaction is spontaneous and $\Delta G = -1.2 \ kcal / mol$
B
Reaction is non spontaneous and $\Delta G = +1.2 \ kcal / mol$
C
Reaction is spontaneous and $\Delta G = -2.4 \ kcal / mol$
D
Reaction is non spontaneous and $\Delta G = +2.4 \ kcal / mol$

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$\Delta H_f^o$ of water is $-285.5\, kJ\, mol^{-1}$. If enthalpy of neutralisation of monoacidic strong base is $-57.3\, kJ\, mol^{-1}$,$\Delta H_f^o$ of $OH^{-}$ ion will be $.....\, kJ\, mol^{-1}$.

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At $1 \ atm$ pressure,$\Delta S = 75 \ J/K \cdot mol$ and $\Delta H = 30 \ kJ/mol$. The temperature of the reaction at equilibrium is $....... \ K$.

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$3 A_{(g)} \rightarrow 2 B_{(g)} + 2 D_{(g)} + E_{(g)}$For the above reaction,$\Delta U = 5.1 \ kcal / mol$ and $\Delta S = 25 \ cal / mol \cdot K$. Which of the following is the correct statement at $300 \ K$?

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$\Delta H_f^o$ of water is $-285.5\, kJ\, mol^{-1}$. If enthalpy of neutralisation of monoacidic strong base is $-57.3\, kJ\, mol^{-1}$,$\Delta H_f^o$ of $OH^{-}$ ion will be $.....\, kJ\, mol^{-1}$.

The enthalpies of combustion of carbon and carbon monoxide are $-393.5 \, kJ \, mol^{-1}$ and $-283 \, kJ \, mol^{-1}$ respectively. The enthalpy of formation of carbon monoxide per mole is $....... \, kJ \, mol^{-1}$. (in $.5$)

At $1 \ atm$ pressure,$\Delta S = 75 \ J/K \cdot mol$ and $\Delta H = 30 \ kJ/mol$. The temperature of the reaction at equilibrium is $....... \ K$.

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$3 A_{(g)} \rightarrow 2 B_{(g)} + 2 D_{(g)} + E_{(g)}$
For the above reaction,$\Delta U = 5.1 \ kcal / mol$ and $\Delta S = 25 \ cal / mol \cdot K$. Which of the following is the correct statement at $300 \ K$?