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?

2.9 g of a gas at 95°C occupied the same volume as 0.184 g of dihydro

1.	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» E gas equation,PV = (w/M) RTSubstituting the given data in the gas equation, we getPV = (2.9 / M) x R x 368&PV = (0.184 / 2) x R x 290From these two equation, we can WRITE(2.9 / M) x R x 368 = (0.184 / 2) x R x 290By, striking THROUG R from both side, we get(2.9 / M) x 368 = (0.184 / 2) x 290Or(2.9 / M) = (0.092 X 290) / 368OrM = 2.9 x 368 / 0.092 x 290= 40 G/molHence, the molar mass of the gas is 40 g mol–1.