The ideal gas law ( <?xml:namespace prefix = v ns = \"urn:schemas-microsoft-com:

Question

The ideal gas law (<?xml:namespace prefix = v ns = "urn:schemas-microsoft-com:vml" /> <?xml:namespace prefix = o ns = "urn:schemas-microsoft-com:office:office" /> PV=nRT ) describes the relationship among pressure P, volume Y, temperature T, and molar amount n. When n and V are fixed, the equation can be rearranged to take the following form where k is a constant:

or(P/T)initial =(P/T)final

When and are fixed, the expression becomes

a)The pressure inside a hydrogen-filled container was 2.10 atm at 21 degre celcius . What would the pressure be if the container was heated to 91degre celcius?

b)At standard temperature and pressure (0  degre celius and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L . What volume would the same amount of gas occupy at the same pressure and 35 degre celcius ?

Explanation / Answer

(A) Thegay-lussacs law:

P1/T1=P2/V2

and temperatures shud be Kelvin (we'll add 273 to the Celcius to get Kelvin)

(2.10atm)/(294K)=(P2)/(364K)

P2= 2.6atm

(B)

P1*V1/T1 = P2*V2/T2

given tha P1 and P2 are equal, these'll cancel out.

so resulting equation

V2 = V1*T2/T1 = 22.4*(273.15+35/(273.15) = 25.27 L

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