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Dalton's Law of Partial Pressures

A quantity of...

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A quantity of an ideal gas is collected in a graduated tube over the mercury in it barometer type arrangement. The volume of the gas at $20^{0}$ C is $50$ ml and the level of mercury is $100$ mm above the outside of the mercury level. The atmospheric pressure is $750$ mm. Volume of gas at STP is? (Take R = $0.083$ it. atmK/mole)

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Solution

$P_{1} = 650 t o r r,$ $V_{1} = 50 m l$ $T_{1} = 20^{0} C + 273 K = 293 K,$ $K P_{2} = 760 T o r r$

$V_{2} = ?,$ $T_{2} = 273 K$

Ideal gas law : $\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$ after rearranging :

$V_{2} = \frac{P_{1} V_{1} T_{2}}{P_{2} T_{1}}$

$= 39.4 m l$ or $40 m l$

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