In Boyles experiment a given gas different temperatures the graph drawn between pressure and density are straight lines as shown then-T-1- - T-2-T-2- - T-1-T-1- - T-2-T-1-3- - T-2-

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Toppr Admin · Accepted Answer

First we derive an expression for density of a gas.
Density $=$ $\frac{m a s s (w)}{v o l u m e (V)}$
but we know that PV $=$ nRT
now, n $=$ $\frac{w}{M}$ where M is molecular weight
So, PV $=$ $\frac{w}{M} R T$
this gives $\frac{w}{V} = \frac{P M}{R T}$ $=$ density $=$ d
so, $P = \frac{d R T}{M}$
so pressure vs density graph will be a straight line with slope $=$ $\frac{R T}{M}$
Hence, steeper the line, more is slope and so more is temperature.
So here $T_{1} > T_{2}$

In Boyles experiment for a given gas at different temperatures the graph drawn between pressure and density are straight lines as shown then:T1>T2T2>T1T1=T2T31=T2

In Boyles experiment for a given gas at different temperatures the graph drawn between pressure and density are straight lines as shown then:

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