For an ideal gas,the V vs T plot at constant | vedclass

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(B) According to the ideal gas equation,$PV = nRT$,which can be rearranged as $V = (nR/P)T$. This is in the form of a straight line equation $y = mx$,

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$P_1 < P_2$

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(B) According to the ideal gas equation,$PV = nRT$,which can be rearranged as $V = (nR/P)T$. This is in the form of a straight line equation $y = mx$,where the slope $m = nR/P$. Since $V$ is plotted against $T$,the slope of the line is $nR/P$. For a given amount of gas ($n$ is constant),the slope is inversely proportional to pressure $(P)$. Therefore,a larger slope corresponds to a smaller pressure. From the figure,the slope of the line for $P_1$ is greater than the slope of the line for $P_2$. Hence,$P_1 < P_2$.

For an ideal gas,the $V$ vs $T$ plot at constant pressures $P_1$ and $P_2$ is shown in the figure. Which of the following is correct?

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