In the given pressure (P) - absolute temperat | vedclass

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(D) For an ideal gas,the equation of state is $PV = nRT$.Rearranging this,we get $P = (nR/V)T$.Comparing this with the equation of a straight line $y

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$V_1 < V_2 < V_3 < V_4$

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(D) For an ideal gas,the equation of state is $PV = nRT$.Rearranging this,we get $P = (nR/V)T$.Comparing this with the equation of a straight line $y = mx$,where $y = P$ and $x = T$,the slope $m$ of the graph is given by $m = nR/V$.Since $n$ and $R$ are constants,the slope is inversely proportional to the volume,i.e.,$m \propto 1/V$.From the given graph,the slope of the line for $V_1$ is the largest,and the slope of the line for $V_4$ is the smallest.Therefore,$m_1 > m_2 > m_3 > m_4$.Since $V \propto 1/m$,it follows that $V_1 < V_2 < V_3 < V_4$.

In the given pressure $(P)$ - absolute temperature $(T)$ graph of an ideal gas,the relation between volumes $V_1, V_2, V_3$ and $V_4$ is

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