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(B) According to Dalton's Law of Partial Pressures,the total pressure is the sum of partial pressures of individual gases.Since the number of molecule

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Decreases to $\frac{650}{2}$

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(B) According to Dalton's Law of Partial Pressures,the total pressure is the sum of partial pressures of individual gases.Since the number of molecules of $N_2$ and $O_2$ are equal,their mole fractions are equal.Therefore,the partial pressure of each gas is half of the total pressure.$P_{total} = P_{N_2} + P_{O_2} = 650 \ mm$Since $P_{N_2} = P_{O_2}$,we have $2 	imes P_{O_2} = 650 \ mm$.Thus,$P_{O_2} = \frac{650}{2} \ mm = 325 \ mm$.If $N_2$ is removed,only $O_2$ remains,and the pressure in the vessel will be the partial pressure of $O_2$,which is $325 \ mm$ or $\frac{650}{2} \ mm$.

$A$ closed vessel contains an equal number of molecules of $N_2$ and $O_2$ at a pressure of $650 \ mm$. If $N_2$ is completely removed,what will be the pressure in the vessel?

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