A gaseous mixture contain oxygen and another unknown gas in molar ratio of 4:1 diffuses through
Answers
Diffusion is the transfer of moles of gas in a specific duraton of time and can be shown as:
d = n /t
where, n is moles of gas
t is time in sec
d1 /d2 = (M2 /M1)1/2 ----(1)
M1 is molar mass of oxygen gas = 32 g /mol
M2 is molar mass of unknown gas
d1 = n /t = 4 /245
d2= 1 /220
Putting the value in (1)
(4*220) /(1*245) = (M2 /32)1/2
3.59 = (M2 /32)1/2
12.89 = M2 /32
M2 = 412.63 g /mol
Hence, molar mass of unknown gas is 412.63 g /mol
Answer:
70.4
Explanation:
let no. of moles of oxygen =4 and no. of moles of unknown gas = 1 and let molecular mass of unknown gas be m
let's first calculate the average molecular mass of the mixture
avg molecular mass= x1m1+x2m2
where x1 and x2 are the mole fraction and m1 and m2 are the molecular mass
so average molecular mass of the mixture = 4/5 x 32 + 1/5 x m
= (128+m)/5
r1/r2=(m2/m1)1
since the same volume of oxygen is used
therefore r1/r2=v/245/v/220 = 220/245 = 44/49
44/49 = ((32 x 5)/(128+m))½
1936/2401=160/(128+m)
247808+1936m= 384160
therefore m = 70.4
so final ans :- 70.4
Thank you