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A and B are ideal gases. The molecular weights of A and B are in the ratio of 1:4 . The pressure of a gas mixture containing equal weights of A and B is P atm. What is the partial pressure (in atm) of B in the mixture ?
\[\begin {array} {1 1} (a)\;\frac{P}{5} & \quad (b)\;\frac{P}{2} \\ (c)\;\frac{P}{2.5} & \quad (d)\;\frac{3P}{4} \end {array}\]
jeemain
eamcet
chemistry
2005
q21
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Nov 8, 2013
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X and Y are two volatile liquids with molar weights of $10\; g\; mol^{–1}$ and $40\; g\; mol^{–1}$ respectively. Two cotton plugs, one soaked in X and the other soaked in Y, are simultaneously placed at the ends of a tube of length $L = 24\; cm$, as shown in the figure. The tube is filled with an inert gas at 1 atmosphere pressure and a temperature of $300\; K$. Vapours of X and Y react to form a product which is first observed at a distance d cm from the plug soaked in X. Take X and Y to have equal molecular diameters and assume ideal behaviour for the inert gas and the two vapours.The experimental value of d is found to be smaller than the estimate obtained using Graham’s law. This is due to:
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