Hi there, I need help with this chemistry gas problem. This is the question: A s

Question

Hi there,

I need help with this chemistry gas problem.

This is the question:

A sample of He gas has a volume of 3720 mL at 1440 torr and -5.32 °C. Calculate the new pressure (in atm), when the temperature of the gas is decreased by 56.0 °C. Assume the volume does not change.

This is my work, and the answer is incorrect. I don't know why:

P1V1/T1 = P2V2/T2

P2= P1V1T2/T1V2

I converted Torr to kPa, degC to K and mL to L. I plugged in the numbers converted kPa to atm, and got 2.40 atm, which is wrong.

Can you help me with this question? Please show your work. Thank you.

Explanation / Answer

P1V1/T1 = P2V2/T2

P2= P1V1T2/T1V2

V = constant

P2 = P1T2 / T1

P2 = (1.895 atm x 211.68K ) / (267.68 )

P2 = 1.49 atm   = 1132.4 torr

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