Question

7.5 g of a gas occupies a volume of 5.6 litres at 0° C and 1 atm pressure. The gas is
(a) NO
(b) N2O
(c) CO
(d) CO2

Answer 1

Answer ⇒ Option (a). 

Given conditions⇒

∵ 5.6 litres of the gas at S.T.P. weighs 7.5 grams.
∴ 1 litres of the gas at S.T.P. weighs 7.5/5.6 grams.
∴ 22.4 litres of the gas at S.T.P. weighs 7.5/5.6 × 22.4 = 30 g.

22.4 litres of the gas at S.T.P. weighs equals to its molar mass.
∴ Molar mass of the gas = 30 g/mole.

For finding the name of the compounds in the given option, Let us first find the molar mass of the compounds. 

Molar mass of the NO = 14 + 16 = 30 g/mole.
Molar mass of the N₂O = 28 + 16 = 44 g/mole.
Molar mass of the O = 14 + 16 = 30 g/mole.
Molar mass of the CO₂ = 14 + 16 × 2 = 44 g/mole.

From this we can see that NO is the correct answer.


Hence Option (a). is correct.


Hope it helps.

Answer 2

Answer:

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