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(B) From the ideal gas equation,$PV = \mu RT = \frac{m}{M}RT$,where $m$ is the mass,$M$ is the molar mass,and $V$ is the volume.Since density $\rho =

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$\frac{273}{373}x$

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(B) From the ideal gas equation,$PV = \mu RT = \frac{m}{M}RT$,where $m$ is the mass,$M$ is the molar mass,and $V$ is the volume.Since density $\rho = \frac{m}{V}$,we can write $P = \frac{\rho RT}{M}$.Therefore,the ratio of density to pressure is $\frac{\rho}{P} = \frac{M}{RT}$.At $0^{\circ}C$ $(T_1 = 273 \ K)$,the ratio is $\left( \frac{\rho}{P} \right)_1 = \frac{M}{R(273)} = x$  --- $(i)$.At $100^{\circ}C$ $(T_2 = 373 \ K)$,the ratio is $\left( \frac{\rho}{P} \right)_2 = \frac{M}{R(373)}$ --- $(ii)$.Dividing equation $(ii)$ by equation $(i)$,we get $\frac{(\rho/P)_2}{x} = \frac{M/R(373)}{M/R(273)} = \frac{273}{373}$.Thus,the ratio at $100^{\circ}C$ is $\frac{273}{373}x$.

At $0^{\circ}C$,the density of a fixed mass of a gas divided by pressure is $x$. At $100^{\circ}C$,the ratio will be

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