The graph drawn between pressure and temperature at constant volume for a given mass of different molecular weights $M_{1}$ and $M_{2}$ are the straight lines as shown in the figure then

M_{2} > M_{1}

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M_{1} > M_{2}

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M_{1} = M_{2}

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M_{1}^{3} = M_{2}

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Solution

The correct option is B $M_{1} > M_{2}$
From ideal gas equation, PV = nRT = $\frac{w}{M} R T$
Slope of P-T curve = $\frac{w R}{M V}$
Since V = constant and w = constant, we get that the slope is inversely proportional to molecular weight
Steeper the line, more is slope, less is molecular weight.
So, $M_{1} > M_{2}$

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The graph drawn between pressure and temperature at constant volume for a given mass of different molecular weights M1 and M2 are the straight lines as shown in the figure then

The correct option is B M1>M2From ideal gas equation, PV = nRT = wMRTSlope of P-T curve = wRMVSince V = constant and w = constant, we get that the slope is inversely proportional to molecular weightSteeper the line, more is slope, less is molecular weight.So, M1>M2

The graph drawn between pressure and temperature at constant volume for a given mass of different molecular weights $M_{1}$ and $M_{2}$ are the straight lines as shown in the figure then