Asample of atmospheric gas collected at an industrial site is stored in a 250 ml amber glass bottle that has a pressure of 1.02 atm and a temperature of 20.3°c. it was placed in an ice chest whose internal temperature is -2.0°c. what will be the new pressure of the gas sample once the gas temperature in the jar equilibrates to that of the ice chest?

The new pressure of the gas sample once the gas temperature in the jar 0.9424 atm.

Explanation:

Volume of the gas = 250 mL

Pressure of the gas at

Pressure of the gas at

At the constant volume pressure of the gas is directly proportional to the temperature of the gas in Kelvins that is Gay-Lussac's Law

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The new pressure of the gas sample once the gas temperature in the jar 0.9424 atm.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.