At STP, weight of $1$ L of a gas is $3.16$ g and weight of $1$ L of hydrogen is $0.09$ g. If molecular weight of hydrogen is $2$ , then the molecular weight of the gas is:

70.8

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

No worries! We‘ve got your back. Try BYJU‘S free classes today!

32.3

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is A 70.8
Vapour density of a gas is the mass of a certain volume of a gas divided by the mass of the same volume of hydrogen gas.

Thus, vapour density of gas $= \frac{3.16}{0.09} = 35.4$ .

Molecular weight is twice the vapour density. Hence, Molecular weight $= 2 \times 35.4 = 70.8$ g/mole.

Suggest Corrections

Similar questions

At STP weight of $1 l i t r e$ of a gas is $3.16 g r a m s$ and weight of $1 l i t r e$ of Hydrogen is $0.09 g m$ . If molecular weight of Hydrogen is 2, molecular weight of the gas is

Q. Density of a gas STP is

1.43 g L^{- 1}

What is its molecular weight?

Q. The density of a gas at STP is

1.5

g/L at STP. Its molecular weight is:

11.2 l

of a gas contains

24 g

of gas at STP. Molecular weight of gas is _________.

Join BYJU'S Learning Program

At STP, weight of 1 L of a gas is 3.16 g and weight of 1 L of hydrogen is 0.09 g. If molecular weight of hydrogen is 2, then the molecular weight of the gas is:

The correct option is A 70.8Vapour density of a gas is the mass of a certain volume of a gas divided by the mass of the same volume of hydrogen gas.Thus, vapour density of gas =3.160.09=35.4.Molecular weight is twice the vapour density. Hence, Molecular weight =2×35.4=70.8 g/mole.

At STP, weight of $1$ L of a gas is $3.16$ g and weight of $1$ L of hydrogen is $0.09$ g. If molecular weight of hydrogen is $2$ , then the molecular weight of the gas is: