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Chemistry

2 litres of a gas is enclosed in a vessel at a pressure of 760 mm Hg. If temperature remains constant, calculate pressure when volume changes to 4 dm3.

Gas Laws

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Answer

V1 = 2 lits.

P1 (Initial pressure) = 760 mm Hg

V2 = 4 dm3

P2 (Final pressure) = ?

By Boyle's Law:

P1V1=P2V2\text{P}1 \text{V}1 = \text{P}2 \text{V}2

Substituting the values :

760×2=P2×4P2=760×24P2=380 mm Hg760 \times 2 = \text{P}2 \times 4 \\[1em] \text{P}2 = \dfrac{760 \times 2}{4} \\[1em] \text{P}_2 = 380 \text{ mm Hg}

∴ Final pressure of the gas = 380 mm Hg.

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