O 2 gas is placed in a 4 litre container containing 3 L of liquid water as shown and total pressure exerted by gases is 720 mm Hg . What will be the pressure of O 2 (g) if given container is attache

Question

O 2 ​ gas is placed in a 4 litre container containing 3 L of liquid water as shown and total pressure exerted by gases is 720 mm Hg . What will be the pressure of O 2 (g) if given container is attached to a empty container of 3 litre at same temperature? Given: [V.P. of H 2 O at 27° C = 20 mm of Hg]

TestHub · Accepted Answer

Question Explanation : Find the pressure of $O_{2} (g)$

Concept : Vapour pressure

Solution : Partial Pressure of $O_{2} (P_{1}) = P_{total} - P_{vap} = 720 - 20 = 700 mm Hg$ $V_{1} =$ Container Volume - Liquid Volume $= 4 L - 3 L = 1 L$

$V_{2} = V_{1} +$ attached empty container volume $= 1 L + 3 L = 4 L$

Since temperature is constant, we can calculate the final partial pressure of $O_{2} (P_{2})$ : $P_{1} \times V_{1} = P_{2} \times V_{2}$

$700 mmHg \times 1 L = P_{2} \times 4 L$

$P_{2} = \frac{700}{4} = 175 mmHg$

Final Answer : Option (A)

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