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3 years ago

A mixture of helium, nitrogen and oxygen has a total pressure of 756 mmHg. The partial

Chemistry

1 answer:

Karolina [17]3 years ago

6 0

Answer:

The partial pressure of oxygen in the mixture is 296 mmHg.

Explanation:

The pressure exerted by a particular gas in a mixture is known as its partial pressure. So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone.

This relationship is due to the assumption that there are no attractive forces between the gases.

So, in this case, the total pressure is:

PT=Phelium + Pnitrogen + Poxygen

You know:

PT= 756 mmHg
Phelium= 122 mmHg
Pnitrogen= 338 mmHg
Poxygen= ?

Replacing:

756 mmHg= 122 mmHg + 338 mmHg + Poxygen

Solving:

756 mmHg - 122 mmHg - 338 mmHg = Poxygen

Poxygen= 296 mmHg

<u><em>The partial pressure of oxygen in the mixture is 296 mmHg.</em></u>

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<h3 /><h3>Reaction stoichiometry</h3>

The balanced reaction is:

3 Cu + 8 HNO₃ → 3 Cu(NO₃)₂ + 2 NO + 4 H₂O

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

Cu: 3 moles
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<h3>Amount of moles of NO produced</h3>

It is possible to determine the the amount of moles of NO produced by a rule of three: if by stoichiometry 8 moles of HNO₃ produce 2 moles of NO, if 27 moles of HNO₃ react how many moles of NO will be formed?

$amount of moles of NO=\frac{27 moles of HNO_{3} x 2 moles of NO}{8 moles of HNO_{3}}$

<u><em>amount of moles of NO= 6.75 moles</em></u>

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