A sample of ammonia gas at 298 K has a volume of 3.5 L at a pressure of 170.2 kPa, what is the new pressure if the gas is compressed to a volume of 1.35 L at 293 K?

The final pressure of the gas comes out to be 433.85 KPa

Explanation:

Initial volume of gas = V = 3.5 L

Initial pressure of gas =  P = 170.2 KPa

Initial temperature = T = 298 K

Final volume of gas = V' = 1.35 L

Final temperature of gas = T' = 293 K

Assuming the number of moles of gas remains constant.

The final pressure of the gas is obtained by the following equation shown below

Final pressure of gas = 433.85 KPa

explanation:

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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