Question

84. Two vessels A and B of 1 litre each contain 0.11 g CO2 gas and 0.07 g of unknown gas respectively under same condition of pressure and temperature then the unknown gas will be

Answer 1

Answer:

28 and unknown gas is N2

Explanation:

Mole of CO2= 0.011/44

=1/400

Mole of CO2= Mole of unknown gas

1/400=Mass/Mw

Mw(molecular mass) =0.07×400

=28

Means unknown gas =N2

Answer 2

Answer:

The unknown gas will be $N_{2}$

Explanation:

We have been given that two vessels A and B of 1 liter each contain $0.11 \ g \ CO_{2}$ gas and $0.07 \ g$ of unknown gas respectively.

The pressure and temperature conditions for both gases are also identical.

We have to find out the unknown gas.

So, moles of $CO_{2}$ = moles of the unknown gas.

Moles of $CO_{2}$ = $\frac{0.011}{44} = \frac{1}{400}$

∴ $\frac{11}{400} = \frac{Mass}{Molecular \ mass}$

Molecular mass = $0.07 \times 400 =28$

We know that $N_{2}$ has a molecular mass of 28 g.

Hence, the unknown gas is $N_{2}$

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