A steel cylinder of internal volume 20 litres is filled with hydrogen at 29 atmospheric pressure. If hydrogen is used to fill a balloon at 1.25 atmospheric pressure at the same temperature, what volume will the gas occupy?

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Solution

According to Boyle's law, $P_{1} V_{1} = P_{2} V_{2}$
if $P_{1} = 29 a t m, V_{1} = 20 l, P_{2} = 1.25 a t m$ , then $V_{2} = \frac{29 \times 20}{1.25} = 464 L$

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A steel cylinder of internal volume 20 litres is filled with hydrogen at 29 atmospheric pressure. If hydrogen is used to fill a balloon at 1.25 atmospheric pressure at the same temperature, what volume will the gas occupy?

According to Boyle's law, P1V1=P2V2if P1=29 atm,V1=20l,P2=1.25 atm, then V2=29×201.25=464 L

According to Boyle's law, $P_{1} V_{1} = P_{2} V_{2}$
if $P_{1} = 29 a t m, V_{1} = 20 l, P_{2} = 1.25 a t m$ , then $V_{2} = \frac{29 \times 20}{1.25} = 464 L$