A sample of gas initially occupies 5.50 L at a pressure of 0.750 atm at 13.0^oC.What will the pressure be if the temperature is changed to 22.5^oC, and the volume is changed to 1.50 L?

Question

Quizplus · Accepted Answer

We can use the combined gas law to solve for the final pressure:

(P1 x V1)/T1 = (P2 x V2)/T2

Where:
P1 = 0.750 atm (initial pressure)
V1 = 5.50 L (initial volume)
T1 = 13.0°C + 273 = 286 K (initial temperature converted to Kelvin)
P2 = ? (final pressure, what we're solving for)
V2 = 1.50 L (final volume)
T2 = 22.5°C + 273 = 296 K (final temperature converted to Kelvin)

Plugging in the values:

(0.750 atm x 5.50 L)/286 K = (P2 x 1.50 L)/296 K

Solving for P2:

P2 = (0.750 atm x 5.50 L x 296 K)/(286 K x 1.50 L)
P2 = 2.84 atm

Therefore, the answer is D) 2.84 atm.

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