(C) Given: $V_1 = 2 \ L$,$V_2 = 2.5 \ L$,$q = +300 \ J$,$P_{ext} = 1 \ atm$. According to the first law of thermodynamics: $\Delta U = q + W$. Work do

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(C) Given: $V_1 = 2 \ L$,$V_2 = 2.5 \ L$,$q = +300 \ J$,$P_{ext} = 1 \ atm$. According to the first law of thermodynamics: $\Delta U = q + W$. Work done $W = -P_{ext} \Delta V = -P_{ext}(V_2 - V_1) = -1 \ atm \times (2.5 \ L - 2 \ L) = -0.5 \ L \cdot atm$. Conversion: $1 \ L \cdot atm = 101.3 \ J$. So,$W = -0.5 \times 101.3 \ J = -50.65 \ J$. Change in internal energy: $\Delta U = 300 \ J + (-50.65 \ J) = 249.35 \ J$.

Class 11 Chemistry Thermodynamics First law of thermodynamics

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$A$ gas occupies $2 \ L$ at $S.T.P.$ It is supplied with $300 \ J$ of heat,causing its volume to expand to $2.5 \ L$ against an external pressure of $1 \ atm$. What is the change in internal energy in $J$?

A
$410.12$
B
$370.34$
C
$249.35$
D
$300.67$

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Thermodynamics

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First law of thermodynamics

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$A$ gas occupies $2 \ L$ at $S.T.P.$ It is supplied with $300 \ J$ of heat,causing its volume to expand to $2.5 \ L$ against an external pressure of $1 \ atm$. What is the change in internal energy in $J$?

Similar Questions

$A$ gas is allowed to expand in an insulated container against a constant external pressure of $10 \ atm$ from an initial volume $4.2 \ L$ to $5.2 \ L$. The change in internal energy $\Delta E$ of the gas will be $:-$

For the reaction $C_{(s)} + O_{2_{(g)}} \rightarrow CO_{2_{(g)}}$,which of the following is true?

The $\Delta U^o$ of combustion of $CH_{4(g)}$ at a certain temperature is $-393 \ kJ/mol$. Then the value of $\Delta H^o$ is:

An ideal gas expands adiabatically against vacuum. Which of the following is correct for the given process?

The enthalpy of vapour is $10 \ kcal/mole$ higher than liquid at $350 \ K$ and $2 \ atm$. Under given conditions,the difference in internal energy of vapour and liquid will be $...... \ cal$.

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