Question:

A 5.00 liter sample of gas measured at 27.0?C and 1.25 atm of pressure has a mass of 10.13 g. What is the mole

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a)39.9

b)0.898

c)2.57

d)2.50 x 10

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  1. I assume that you want to know the molecular mass of the gas.

    PV = nRT

    126.625 * 5 = n * 8.31*300

    n = 126.625*5/8.31*300

    n = 0.254 moles

    Mass is 10.13, therefore molar mass = 10.13/0.254 = 39.9

    Answer is a) above.


  2. Assuming this is an ideal gas, you can use the equation

    PV = nRT

    where P = pressure ( atm )

    V = vol ( L )

    T = temperature ( ºK ) , R = universal gas constant = 0.08205

    n= no of moles

    therefore solving for n ,

    n = PV / RT

    n = ( 1.25 ) ( 5 ) / ( 0.08205 ) ( 27 + 273 )

    n = 0.25 moles

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