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Chapter 8: Problem 59

A sample of ozone gas is found to be \(40 \%\) dissociated into oxygen. The average molecular mass of sample should be

Short Answer

Expert verified
Answer: The average molecular mass of the ozone sample is 41.6 g/mol.

Step by step solution

01

Identify the mass of ozone and oxygen molecules

To find the average molecular mass of the sample, we first need to know the molecular weights of ozone and oxygen. The molecular weight of an oxygen atom is 16 g/mol. The molecular weight of ozone (O3) is 3 times the atomic weight of oxygen, and the molecular weight of oxygen (O2) is 2 times the atomic weight of oxygen. So, the molecular weight of ozone (O3) is: #\( 3 \times 16 \)= 48 g/mol#. The molecular weight of oxygen (O2) is: #\( 2 \times 16 \)= 32 g/mol#.
02

Calculate the proportional mass of ozone and oxygen molecules

We know that the sample of ozone is 40% dissociated into oxygen. Therefore, 60% of the sample remains ozone, and 40% of the sample is now oxygen. Proportional mass of ozone in the sample: #0.6 \times 48 g/mol = 28.8 g/mol#. Proportional mass of oxygen in the sample: #0.4 \times 32 g/mol = 12.8 g/mol#.
03

Calculate the average molecular mass of the sample

To find the average molecular mass of the sample, we will add the proportional mass of both ozone and oxygen molecules. Average molecular mass of the sample: #28.8 + 12.8 = 41.6 g/mol#. So, the average molecular mass of the given ozone sample, which is 40% dissociated into oxygen, is 41.6 g/mol.

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Most popular questions from this chapter

It was found from the chemical analysis of a gas that it has two hydrogen atoms for each carbon atom. At \(0^{\circ} \mathrm{C}\) and \(1 \mathrm{~atm}\), its density is \(1.25 \mathrm{~g}\) per litre. The formula of the gas would be (a) \(\mathrm{CH}_{2}\) (b) \(\mathrm{C}_{2} \mathrm{H}_{4}\) (c) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (d) \(\mathrm{C}_{4} \mathrm{H}_{8}\)

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