(A) According to the first law of thermodynamics,$\Delta U = q + w$. Given: Heat supplied $q = +300 \ J$. Pressure $P = 1 \ atm$. Initial volume $V_1

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(A) According to the first law of thermodynamics,$\Delta U = q + w$. Given: Heat supplied $q = +300 \ J$. Pressure $P = 1 \ atm$. Initial volume $V_1 = 1.5 \ L$,Final volume $V_2 = 2 \ L$. Change in volume $\Delta V = V_2 - V_1 = 2 - 1.5 = 0.5 \ L$. Work done $w = -P \Delta V = -1 \ atm \times 0.5 \ L = -0.5 \ L \cdot atm$. Since $1 \ L \cdot atm = 101 \ J$,then $w = -0.5 \times 101 \ J = -50.5 \ J$. Now,$\Delta U = 300 \ J - 50.5 \ J = 249.5 \ J$.

Class 11 Chemistry Thermodynamics First law of thermodynamics

Medium

The volume of a gas at $STP$ is $1.5 \ L$. When $300 \ J$ of heat is supplied to it at $1 \ atm$ pressure,its volume becomes $2 \ L$. What is the value of $\Delta U$ in $J$ for this process? $(1 \ L \cdot atm = 101 \ J)$

A
$249.5$
B
$236.8$
C
$246.8$
D
$160.8$

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First law of thermodynamics

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One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of $27\, ^{\circ}C$. If the work done during the process is $3\, kJ$,then the final temperature of the gas is $(C_v = 20\, J\, K^{-1}\, mol^{-1})$ .....$K$

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For the gas phase reaction $A_{2(g)} + B_{2(g)} \rightarrow 2AB_{(g)}$ taking place at constant pressure and temperature where all gases are behaving ideally,which of the following must be correct?

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The volume of a gas at $STP$ is $1.5 \ L$. When $300 \ J$ of heat is supplied to it at $1 \ atm$ pressure,its volume becomes $2 \ L$. What is the value of $\Delta U$ in $J$ for this process? $(1 \ L \cdot atm = 101 \ J)$

Similar Questions

Assertion : For a reaction $2NH_{3(g)} \to N_{2(g)} + 3H_{2(g)}$ ; $\Delta H > \Delta E$.Reason : Enthalpy change is always greater than internal energy change.

One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of $27\,^{\circ}C$. If the work done during the process is $3\, kJ$,then the final temperature of the gas is $(C_v = 20\, J/K)$ .....$K$

One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of $27\, ^{\circ}C$. If the work done during the process is $3\, kJ$,then the final temperature of the gas is $(C_v = 20\, J\, K^{-1}\, mol^{-1})$ .....$K$

For the gas phase reaction $A_{2(g)} + B_{2(g)} \rightarrow 2AB_{(g)}$ taking place at constant pressure and temperature where all gases are behaving ideally,which of the following must be correct?

What is the amount of work done when $0.5 \ mol$ of methane,$CH_{4(g)}$,is subjected to combustion at $300 \ K$? (Given: $R = 8.314 \ J \ K^{-1} \ mol^{-1}$)

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Assertion : For a reaction $2NH_{3(g)} \to N_{2(g)} + 3H_{2(g)}$ ; $\Delta H > \Delta E$.
Reason : Enthalpy change is always greater than internal energy change.