Question

2.9 g of a gas at 95°C occupied the same volume as 0.184 g of dihydrogen at 17°C, at the same pressure. What is the molar mass of the gas?

Answer 1

From the gas equation,

PV = (w/M) RT

Substituting the given data in the gas equation, we get

PV = (2.9 / M) x R x 368

&

PV = (0.184 / 2) x R x 290

From these two equation, we can write

(2.9 / M) x R x 368 = (0.184 / 2) x R x 290

By, striking throug R from both side, we get

(2.9 / M) x 368 = (0.184 / 2) x 290

Or

(2.9 / M)   =  (0.092 X 290) / 368

Or

M  = 2.9 x 368 / 0.092 x 290

= 40 g/mol

Hence, the molar mass of the gas is 40 g mol–1.

Answer 2

HLO MATE HERE U GO

⭐. Gas equation is PV = nRT

when volume and pressure of two gases are same then ,

n1T1 = n2 T2 ==> w1/M1 × T 1 = w2/ M2 × T2

==> M1 = M2 w1T1 / W2 T2

==> 2× 2.9 × 368 / 0.184 × 290

==> 40 g /mol.