At 298 K, a flask 'A' of unknown volume (V) | vedclass

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(B) Using the ideal gas equation $PV = nRT$, the number of moles of oxygen in flask '$A$' is $n_{O_2} = \frac{P_A V_A}{RT} = \frac{5 	imes V}{RT}$.Si

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$0.3$

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(B) Using the ideal gas equation $PV = nRT$, the number of moles of oxygen in flask '$A$' is $n_{O_2} = \frac{P_A V_A}{RT} = \frac{5 	imes V}{RT}$.Similarly, the number of moles of helium in flask '$B$' is $n_{He} = \frac{P_B V_B}{RT} = \frac{3 	imes 2}{RT} = \frac{6}{RT}$.The mole fraction of oxygen in the mixture is given by $x_{O_2} = \frac{n_{O_2}}{n_{O_2} + n_{He}} = 0.2$.Substituting the values: $\frac{5V/RT}{5V/RT + 6/RT} = 0.2$.This simplifies to $\frac{5V}{5V + 6} = 0.2$.$5V = 0.2(5V + 6) \implies 5V = V + 1.2$.$4V = 1.2 \implies V = 0.3 \ L$.

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