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

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

Question

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

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

Toppr Admin · Accepted Answer

From 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-gt-M2

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 M2>M1M1>M2M1=M2M31=M2

From 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

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

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, $M_{1} > M_{2}$