What pressure (in ATM) is exerted by a mixture of 2g of H2 and 8g of N2 at 273 in 10L container? Given that:[ H=1: N=14;Molar gas constant,R=0.0821 atmLmol]

1 Answer
Mar 25, 2018

#P~=3*atm#

Explanation:

#"Moles of dihydrogen"=(2.0*g)/(2.016*g*mol^-1)=0.992*mol#

#"Moles of dinitrogen"=(8.0*g)/(28.02*g*mol^-1)=0.286*mol#

#n_"total moles of gas"=n_"dinitrogen"+n_"dihydrogen"=1.278*mol#

And we use the old Ideal Gas equation...

#P=(n_"total"RT)/V=(1.278*molxx0.0821*(L*atm)/(K*mol)xx273.15*K)/(10*L)#

#-=??*atm#