Two moles of an ideal gas is expanded isothermally from a volume of $300 \ cm^3$ to $2.5 \ dm^3$ at $298 \ K$ against a constant pressure of $1.9 \ bar$. Calculate the work done in joules. (in $J$)
- A$-418$
- B$-565$
- C$-918$
- D$-950$
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$1 \, mol$ of an ideal gas is compressed reversibly at a constant temperature of $27 \, ^oC$ from $1 \, bar$ to $4 \, bar$. Calculate the work done in $kJ$.
Medium
View SolutionThe enthalpy change $(\Delta H)$ for the reaction,$N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$ is $-92.38 \ kJ$ at $298 \ K$. The internal energy change $\Delta U$ at $298 \ K$ is .............. $kJ$
MediumAIIMS 2006
View SolutionTwo mole of an ideal gas is expanded isothermally and reversibly from $1 \ L$ to $10 \ L$ at $300 \ K$. The enthalpy change (in $kJ$) for the process is .....$kJ$
Observe the following properties:
$I$. Molar volume
$II$. Mass
$III$. Internal energy
$IV$. Volume
$V$. Enthalpy
$VI$. Temperature
$VII$. Density
The intensive properties in the above list are:
$I$. Molar volume
$II$. Mass
$III$. Internal energy
$IV$. Volume
$V$. Enthalpy
$VI$. Temperature
$VII$. Density
The intensive properties in the above list are:
$A$ thermodynamic process $(B \rightarrow E)$ is shown in the graph below. The work done in this process is equal to the area under the curve. Identify the correct area representing the work done.
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