For many purposes we can treat nitrogen as an ideal gas at temperatures above its boiling point of . Suppose the temperature of a sample of nitrogen gas is raised from to , and at the same time the pressure is changed. If the initial pressure was and the volume decreased by , what is the final pressure? Round your answer to significant digits.

12.3 atm

Explanation:

In this question, the following gas parameters are mentioned;

Temperature, Pressure and Volume

The relationship between all three parameters is given by the general gas equation;

V1P1 / T1 =V2P2 / T2

From the question;

P1 initial pressure = 7atm

P2 final pressure = ?

T1 initial temperature = - 13°C + 273 = 260K (converting to kelvin temperature)

T2 final  temperature = 24°C + 273 =297K (converting to kelvin temperature)

The volume decreased by 35%

V1 initial volume = 100 dm3

V2final  volume = 100 - 35 = 65 dm3

Substituting all the values into the equation, we have;

7 * 100 / 260 = P2 * 65 / 297

P2 * 65 * 260 = 7 * 100 * 297

P2 = 207900 / 16900 = 12.3 atm

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