(A) For an isothermal reversible expansion process,the work done is given by the formula:$W = -2.303 \, nRT \log \left( \frac{V_2}{V_1} \right)$Given:

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$-2.303 \times 8.314 \times 10^7 \times 298 \log(2)$

(A) For an isothermal reversible expansion process,the work done is given by the formula:$W = -2.303 \, nRT \log \left( \frac{V_2}{V_1} \right)$Given:$n = 1 \, \text{mole}$$T = 25 + 273 = 298 \, K$$V_1 = 10 \, L, V_2 = 20 \, L$$R = 8.314 \times 10^7 \, erg \, K^{-1} \, mol^{-1}$ (since the answer is required in $erg$)Substituting the values:$W = -2.303 \times 1 \times (8.314 \times 10^7) \times 298 \log \left( \frac{20}{10} \right)$$W = -2.303 \times 8.314 \times 10^7 \times 298 \log(2) \, erg$

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

What is the work done in $erg$ for the reversible expansion of $1 \, \text{mole}$ of an ideal gas from $10 \, L$ to $20 \, L$ at $25 \, ^oC$?

A
$-2.303 \times 8.314 \times 10^7 \times 298 \log(2)$
B
$-2.303 \times 8.314 \times 298 \log(2)$
C
$2.303 \times 8.314 \times 10^7 \times 298 \log(0.5)$
D
$2.303 \times 8.314 \times 298 \log(2)$

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Thermodynamics

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Mix Examples-Thermodynamics and Thermochemistry

Which of the following is/are true about the reversible isothermal expansion of an ideal gas?
$(a) \ \Delta U = 0$
$(b) \ q = 0$
$(c) \ \Delta T = 0$
$(d) \ q = 2.303 \ nRT \ \log_{10} \left( \frac{V_2}{V_1} \right)$

Medium

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$A$ calorimeter contains $0.2 \ kg$ of water at $30^{\circ} C$. $0.1 \ kg$ of water at $60^{\circ} C$ is added to it,the mixture is well stirred and the resulting temperature is found to be $35^{\circ} C$. The water equivalent of the calorimeter is $:-$ (in $J / K$)

Medium

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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 $....... \ K$.

Easy

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Calculate $\Delta H_f^o$ of $SiH_2$ from the following reactions:
$Si_2H_{6(g)} + H_{2(g)} \to 2SiH_{4(g)}, \Delta H = -11.7 \ kJ/mol$
$SiH_{4(g)} \to SiH_{2(g)} + H_{2(g)}, \Delta H = +239.7 \ kJ/mol$
$\Delta H_f^o(Si_2H_{6(g)}) = 80.3 \ kJ/mol$

Medium

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Match the conditions and the temperature for the 'fusion' process of $H_2O_{(s)}$ at $1 \ atm$ pressure.

Condition Temperature

$(1)$. Spontaneous $(p)$. $273 \ K$

$(2)$. At equilibrium $(q)$. $260 \ K$

$(3)$. Non-spontaneous $(r)$. $280 \ K$

Condition	Temperature
$(1)$. Spontaneous	$(p)$. $273 \ K$
$(2)$. At equilibrium	$(q)$. $260 \ K$
$(3)$. Non-spontaneous	$(r)$. $280 \ K$

Medium

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What is the work done in $erg$ for the reversible expansion of $1 \, \text{mole}$ of an ideal gas from $10 \, L$ to $20 \, L$ at $25 \, ^oC$?

Similar Questions

Which of the following is/are true about the reversible isothermal expansion of an ideal gas?$(a) \ \Delta U = 0$$(b) \ q = 0$$(c) \ \Delta T = 0$$(d) \ q = 2.303 \ nRT \ \log_{10} \left( \frac{V_2}{V_1} \right)$

$A$ calorimeter contains $0.2 \ kg$ of water at $30^{\circ} C$. $0.1 \ kg$ of water at $60^{\circ} C$ is added to it,the mixture is well stirred and the resulting temperature is found to be $35^{\circ} C$. The water equivalent of the calorimeter is $:-$ (in $J / K$)

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 $....... \ K$.

Calculate $\Delta H_f^o$ of $SiH_2$ from the following reactions:$Si_2H_{6(g)} + H_{2(g)} \to 2SiH_{4(g)}, \Delta H = -11.7 \ kJ/mol$$SiH_{4(g)} \to SiH_{2(g)} + H_{2(g)}, \Delta H = +239.7 \ kJ/mol$$\Delta H_f^o(Si_2H_{6(g)}) = 80.3 \ kJ/mol$

Match the conditions and the temperature for the 'fusion' process of $H_2O_{(s)}$ at $1 \ atm$ pressure. Condition Temperature $(1)$. Spontaneous $(p)$. $273 \ K$ $(2)$. At equilibrium $(q)$. $260 \ K$ $(3)$. Non-spontaneous $(r)$. $280 \ K$

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Which of the following is/are true about the reversible isothermal expansion of an ideal gas?
$(a) \ \Delta U = 0$
$(b) \ q = 0$
$(c) \ \Delta T = 0$
$(d) \ q = 2.303 \ nRT \ \log_{10} \left( \frac{V_2}{V_1} \right)$

Calculate $\Delta H_f^o$ of $SiH_2$ from the following reactions:
$Si_2H_{6(g)} + H_{2(g)} \to 2SiH_{4(g)}, \Delta H = -11.7 \ kJ/mol$
$SiH_{4(g)} \to SiH_{2(g)} + H_{2(g)}, \Delta H = +239.7 \ kJ/mol$
$\Delta H_f^o(Si_2H_{6(g)}) = 80.3 \ kJ/mol$

Match the conditions and the temperature for the 'fusion' process of $H_2O_{(s)}$ at $1 \ atm$ pressure.

Condition Temperature

$(1)$. Spontaneous $(p)$. $273 \ K$

$(2)$. At equilibrium $(q)$. $260 \ K$

$(3)$. Non-spontaneous $(r)$. $280 \ K$