At 25 , ^circ C,the density of oxygen gas is | vedclass

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(B) According to the ideal gas equation,$PV = nRT = (m/M)RT$,where $P$ is pressure,$V$ is volume,$m$ is mass,$M$ is molar mass,$R$ is the gas constant

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$2 \, atm$

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(B) According to the ideal gas equation,$PV = nRT = (m/M)RT$,where $P$ is pressure,$V$ is volume,$m$ is mass,$M$ is molar mass,$R$ is the gas constant,and $T$ is temperature. Rearranging for density $(d = m/V)$,we get $P = (dRT)/M$. Since $R$,$T$,and $M$ are constant for a given gas at a constant temperature,the pressure $P$ is directly proportional to the density $d$ $(P \propto d)$. Given that the initial density $d_1 = 1.458 \, mg/L$ at $P_1 = 1 \, atm$,if the new density $d_2 = 2 	imes d_1$,then the new pressure $P_2$ will be $2 	imes P_1$. Therefore,$P_2 = 2 	imes 1 \, atm = 2 \, atm$.

At $25 \, ^\circ C$,the density of oxygen gas is $1.458 \, mg/L$ at $1 \, atm$ pressure. What will be the pressure of oxygen gas if the density is doubled?

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