A gas cylinder containing 1.50 mol compressed methane has a volume of 3.30 L. Wh

Question

A gas cylinder containing 1.50 mol compressed methane has a volume of 3.30 L. What pressure does the methane exert on the walls of the cylinder if its temperature is 25 A gas cylinder containing 1.50 mol compressed methane has a volume of 3.30 L. What pressure does the methane exert on the walls of the cylinder if its temperature is 25 A gas cylinder containing 1.50 mol compressed methane has a volume of 3.30 L. What pressure does the methane exert on the walls of the cylinder if its temperature is 25

Explanation / Answer

The ideal gas law is:

PV=nRT where P - pressure, V - volume, n - number of moles, R - gas constant, and T - temperature.

The value of R is 0.08205746 (L*atm)/(K*?mol) (That is according to wikipedia but I believe it's correct.)

Now lets rearrange the ideal gas law to solve for pressure:

P=(nRT)/V

Now just plug and chug...

P=(1.50moles * 0.08205746(L*atm)/(K*?mol) * (273.15+25)K)/3.30L = 11.12atm

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