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Ideal Gas Equation

The absolute ...

Question

The absolute temperature T of a gas is plotted against its pressure P for two different constant volumes V $_{1}$ and V $_{2}$ where V $_{1}$ > V $_{2}$ . T is plotted along x-axis and P along y-axis.

Slope for curve corresponding to volume V

_{1}

is greater than that corresponding to volume V

_{2}

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Slope for curve corresponding to volume V

_{2}

is greater than that corresponding to volume V

_{1}

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Slope for both curves are equal.

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Slope for both curves are unequal such that they intersect at T = 0.

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Solution

The correct option is B Slope for curve corresponding to volume V $_{2}$ is greater than that corresponding to volume V $_{1}$ .
From ideal gas equation, PV = nRT
This means that $P = \frac{n R}{V} T$
So, the slope of P-T curve = $\frac{n R}{V} α \frac{1}{V}$
this means that more slope => less volume
Since we are given that $V_{2} < V_{1}$ , so we get that
Slope for curve corresponding to volume $V_{2}$ is greater than that corresponding to volume $V_{1}$ .
So, B is the correct answer.

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The absolute temperature T of a gas is plotted against its pressure P for two different constant volumes V1 and V2 where V1 > V2. T is plotted along x-axis and P along y-axis.

The absolute temperature T of a gas is plotted against its pressure P for two different constant volumes V $_{1}$ and V $_{2}$ where V $_{1}$ > V $_{2}$ . T is plotted along x-axis and P along y-axis.