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A sample of a diatonic gas is loaded into an evacuated bottle at STP. The 0.25 L bottle contains 1.76 grams of the unidentified gas. Calculate the molar mass of the gas. What is the identity of the diatomic gas?

Answers

Answer 1

Answer:

(a) 157.7 g

(b) 7.04 g/dm³

Explanation:

(a) From the question,

According to Avogadro's Law,

1 mole of every gas at STP occupies a volume of 22.4 dm³

But mass of 1 mole of the diatomic gas  = molar mass of the gas.

This Implies that,

The molar mass of the gas at STP occupies a volume of 22.4 dm³

From the question,

If,

0.25 L bottle contain 1.76 g of the gas,

Therefore,

Molar mass of the gas = (1.76×22.4)/0.25

Molar mass of the gas = 157.7 g.

(b) Density of the gas = mass/volume

D = m/v

Given: m = 1.76 g, v = 0.25 L = 0.25 dm³

Therefore,

D = 1.76/0,25

D = 7.04 g/dm³

Related Questions

In calorimetry, energy is measured through heat transfer from one substance to
another. Which of the following is NOT a method of heat transfer?

Answers

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Answer:

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