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(A) From the ideal gas equation,$PV = nRT = \frac{w}{M}RT$,we have $P = \frac{dRT}{M}$,where $d$ is the density,$R$ is the gas constant,$T$ is the tem

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$1:1$

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(A) From the ideal gas equation,$PV = nRT = \frac{w}{M}RT$,we have $P = \frac{dRT}{M}$,where $d$ is the density,$R$ is the gas constant,$T$ is the temperature,and $M$ is the molar mass.For the same gas,$M$ is constant,so $P \propto dT$.Therefore,the ratio of pressures is $\frac{P_1}{P_2} = \frac{d_1}{d_2} 	imes \frac{T_1}{T_2}$.Given $\frac{d_1}{d_2} = \frac{1}{2}$ and $\frac{T_1}{T_2} = \frac{2}{1}$.Substituting these values,$\frac{P_1}{P_2} = \frac{1}{2} 	imes \frac{2}{1} = \frac{1}{1}$.Thus,the ratio of their respective pressures is $1:1$.

Densities of a gas at different conditions are in the ratio $1:2$ and their temperatures are in the ratio $2:1$,then the ratio of their respective pressure is :-

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