$A$ 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 $:-$
- A$+1013 \ J$
- B$+10 \ atm \cdot L$
- C$-1013 \ atm \cdot L$
- D$-1013 \ J$
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Similar Questions
If $3 \ mol$ of an ideal gas at $300 \ K$ expand isothermally from $30 \ dm^3$ to $45 \ dm^3$ against a constant opposing pressure of $80 \ kPa$,then the amount of heat transferred is . . . . . . $J$.
DifficultJEE MAIN 2024
View SolutionWhat is the amount of work done when $0.5 \ mol$ of methane,$CH_{4(g)}$,is subjected to combustion at $300 \ K$? (Given: $R = 8.314 \ J \ K^{-1} \ mol^{-1}$)
For an ideal gas,the heat of reaction at constant pressure and heat of reaction at constant volume are related by the equation:
$A$ gas performs $0.320 \ kJ$ work on the surrounding and absorbs $120 \ J$ of heat from the surrounding. Hence,the change in internal energy is: (in $J$)
The first law of thermodynamics for an isothermal process is:
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