A 3.00-L sample of helium at 0.00°C and 1.00 atm is compressed into a 0.50-L cylinder. What pressure will the gas exert in the cylinder at 50.°C?

P = 7.1 atm

Explanation: For this problem we will use Combined Gas Law to solve for the new pressure. But never forget to convert the unit of temperature to Kelvin.

P1V1 /T1 = P2V2/ T2, Derive for P2.

P2 = P1V1T2 / T1V2

= 1.00 atm ( 3.00 L ) ( 323 K) / 273 K ( 0.50 L )

= 7.1 atm

Cancel out the units of L and K and the unit remains is in atm.

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