A 1.54L gas bulb in a chemistry laboratory contains oxygen gas at 21 degrees C and 758 torr. The air conditioning in the laboratory breaks down (cause ... You know ... It's Morehouse) and the temperature rises to 31 degrees. Calculate the final pressure of the gas given this increase in temperature

Question

Chemistry

Ferris

21 February, 14:28

A 1.54L gas bulb in a chemistry laboratory contains oxygen gas at 21 degrees C and 758 torr. The air conditioning in the laboratory breaks down (cause ... You know ... It's Morehouse) and the temperature rises to 31 degrees. Calculate the final pressure of the gas given this increase in temperature

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Answers (1)

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Marley Monroe · Answer 1

784 torr

Explanation:

Using Pressure Law; at constant volume,

P∝ T at constant volume.

P = kT; meaning

P1/T1 = P2/T2

P1 = 758 torr

P2=?

T1 = 21 ° C or (273+21) K

= 294°K

T2 = 31 ° C or (273+31) K

= 304°K

Substituting into equation (1),

We have:

758/294 = P2/304

P2 = 758 x 304/294

= 783.78torr

≈ 784 torr