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

70.8

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64.4

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32.2

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44.6

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Solution

The correct option is A
70.8

V.D. = $\frac{W e i g h t o f^{'} x^{'} m l o f a g a s}{W e i g h t o f^{'} x^{'} m l o f H_{2} g a s}$

= $\frac{3.16}{0.09} = 35.4$

M.W. = $2 \times V D = 70.8$

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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. 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:

5

litre of gas at STP weights

6.25 g

. What is its gram molecular weight?

Q. At

S T P

, the density of a gas (molecular weight 45) in grams per litre is:

Q. At

S T P

weight of 1 litre of a gas is

1.25

grams. The gas will be:

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At STP weight of 1 litre of a gas is 3.16 grams and weight of 1 litre of Hydrogen is 0.09 gm. If molecular weight of Hydrogen is 2, molecular weight of the gas is

The correct option is A 70.8 V.D. = Weight of ′x′ ml of a gasWeight of ′x′ ml of H2 gas = 3.160.09 = 35.4 M.W. = 2 × VD = 70.8

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

The correct option is A
70.8

V.D. = $\frac{W e i g h t o f^{'} x^{'} m l o f a g a s}{W e i g h t o f^{'} x^{'} m l o f H_{2} g a s}$

= $\frac{3.16}{0.09} = 35.4$

M.W. = $2 \times V D = 70.8$