The work done during the expansion of a gas from a volume of $4 \ dm^3$ to $6 \ dm^3$ against a constant external pressure of $3 \ atm$ is $(1 \ L \ atm = 101.32 \ J)$ $...... \ J$
- A$+ 304$
- B$-304$
- C$-6$
- D$-608$
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Similar Questions
$1 \ mol$ of an ideal gas is allowed to expand isothermally and reversibly from $1 \ L$ to $5 \ L$ at $300 \ K$. The change in enthalpy (in $kJ$) is $(R = 8.3 \ J \ K^{-1} \ mol^{-1})$.
Which from the following defines enthalpy of a system?
Two moles of an ideal gas expand freely and isothermally from $5 \ dm^3$ to $50 \ dm^3$. What is the value of $\Delta H$?
$A$ given mass of gas expands from state $A$ to state $B$ by three paths $1, 2$ and $3$ as shown in the figure. If $w_1, w_2$ and $w_3$ are the work done by the gas along the three paths respectively,then:
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View SolutionFor an ideal gas,the heat of reaction at constant pressure and constant volume are related as:
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