Sample 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?

- New pressure is 0.942 atm.

Solution:- The volume of the glass bottle would remain constant here and the pressure will change with the temperature.

Pressure is directly proportional to the kelvin temperature. The equation used here is:

Where, and are initial and final temperatures, and are initial and final pressures.

= 20.3 + 273.15 = 293.45 K

= -2.0 + 273.15 = 271.15 K

= 1.02 atm

 = ?

Let's plug in the values in the equation and solve it for final pressure.

= 0.942 atm

So, the new pressure of the jar is 0.942 atm.

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in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm