chemistry question help

Question

A sample of argon gas occupies a volume of 0.0450 m^3 at 101.3 kPa and 25.0∘C. What volume would the same sample of gas occupy if the pressure was increased to 161.0 kPa at constant temperature.

Answer 1

V1 = initial volume = 0.0450 m³ x 1000 L / m³ = 45.0 L

P1 = initial pressure = 101.3 kPa

T1 = initial temperature in Kelvin = 25.0ºC + 273 = 298K

V2 = final volume = ?

P2 = final pressure = 161.0 kPa

T2 = final temperature = 298K

Since T is constant, we are dealing with Boyle's law:

P1V1 = P2V2

101.3 kPa / 45.0 L = 161 kPa / V2

V2 = (45 L)(161 kPa) / 101.3 kPa)

V2 = 71.5 L

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If you choose not to change m³ to liters, you have

V2 = (0.0450 m³)(161 kPa) / 101.3 kPa

V2 = 0.0715 m³

Answer 2

The process for this question is very similar to what I explained here: https://www.wyzant.com/resources/answers/912285/help-with-chemistry

Note that in this question, you have different types of units for volume (cubic meters) and pressure (kPa), but the approach is the same.