Homework Answers
Step 1: Initial given pressure is 2.35 atm, for 1.5 L volume and 250C temperature.
Step 2: If the volume of the container is reduced to 1:00 L at constant temperature, then according to Boyles law:
P1V1 = P2V2
P2 = P1V1/V2 .( Where P1= initial pressure; P2 = final pressure; V1 = initial volume and V2 = final volume)
P2 = 2.35 atm X 1.5 L / 1 L
P2 = 3.525 atm.
Step 3: If the temperature is raised, by keeping the volume constant, then according to Gay-Lussac's law, the pressure of a gas is directly proportional to the temperature in Kelvin.
Therefore,
P1/T1. = P2/T2
P2 = P1 X T2/T1
P2 = 2.35 atm X 310.4 k/ 298k
P2 = 2.447 atm.
The increase in pressure is more in first case, rather than second case, hence, keeping the gas in the container of volume 1L is more hazardous, where there are more chances of explosion.
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