At a constant temperature a certain mass of gas occupies 7.5It when the pressure is 800 mm of Hg. Calculate the pressure at which the volume of the gas would be decreases by 35% of its initial volume.

Q. A gas occupies

V

litres at a certain temperature. Keeping its pressure constant, its volume can be reduced to half its initial volume at

27^{o} C

. The original temperature of the gas is:

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The volume of the gas is to be found at a pressure of 2500Pa. when the pressure was decreased by 500Pa the gas occupied a volume of 2400 litres. Calculate the initial volume occupied by gas before the change was done while maintaining a constant pressure constant temperature?

The correct option is B 1920 litres P1= 2500,P2= 2500-500 = 2000,V2 = 2400,V1=? According to Boyle's law P1V1 = P2V2 (at constant temperature) 2500×V1=2000×2400 V1= 1920 litres

The correct option is B
1920 litres

$P_{1}$ = 2500, $P_{2}$ = 2500-500 = 2000, $V_{2}$ = 2400, $V_{1}$ =?

According to Boyle's law

$P_{1} V_{1}$ = $P_{2} V_{2}$ (at constant temperature)

$2500 \times V_{1} = 2000 \times 2400$

$V_{1}$ = 1920 litres