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4 Questions around this concept.
One mole of an ideal gas expands from state X to Y by three paths 1, 2 and 3 as shown in the figure below. If W1, W2 and W3 are respective work done by ideal gas along the three paths then:
What is the relation between the temperatures in the below graph which represents isothermal expansion of gas at different temperatures?
when will a sample of Diatomic gas is consider at a initial Pressure of 80 kPa . The volume of gas is then compressed from $900 \mathrm{~cm}^3$ to $300 \mathrm{~cm}^3$ adiabatically. find the value of workdone on the gas will be.
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1. Constant Volume Process:
Representation on P-V diagram:
This process is represented on the P-V diagram by a vertical straight line as shown in figure, since V1=V2.
Work done during the process:
$\mathrm{W}=\int_{\mathrm{V}_1}^{\mathrm{V}_2} \mathrm{Pdv}$
But $\mathrm{dv}=0$ for an isochoric process
$\therefore W=0$
Thus, work done during constant volume process is zero which is also evident from the P-V diagram as no area is enclosed by the vertical line on P-V diagram.
2. Constant Pressure Process:
Representation on P-V diagram:
During this process the pressure or the gas remains constant therefore it is represented by a horizontal line on P-V diagram. See figure.
Work done during the process:
$
\mathrm{W}=\int_{\mathrm{V}_1}^{\mathrm{V}_2} \mathrm{Pdv}
$
But P is constant.
$\therefore$ Work done $=P \int_{V_1}^{V_2} d v=P\left(V_2-V_1\right)$
The work done by the gas during constant pressure process is represented by a rectangle on P-V diagram.
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