Question

16g of oxygen and 14g of nitrogen mixed in 5000cm at 300 k resulting pressure

Answer 1

Answer:

use formula substitute and find out

Explanation:

Answer 2

Answer:

Concept:

According to Dalton's law of level of oxygen, the overall pressure placed by a mixture of gases is equal to the sum of the partial pressures of all the individual gases, and each gas is regarded an Ideal gas. The partial pressures of gas 1, gas 2, and gas 3 are P1, P2, and P3, respectively.

Given:

16 g of oxygen and 14 g of nitrous mixed in 5000cm at 300 k resulted in a pressure 

Find:

find the pressure of a mixture

Answer:

Partial pressures can be calculated in two ways:

1)To compute the individual pressure of each gas in a mixture, use

$PV = nRT$

2)Calculate the percentage of stress from the pressure head addressable to each individual gas using the mole fraction of each gas.

$PV=nRT$

$nO_{2} =\frac{16}{32}$

       $=0.5$

$nN2 = \frac{14}{28}$

       $=0.5$

$p=\frac{nRT}{v}$

  $=\frac{1*8.3*300}{5*10^{-3} }$

$p = 498000 pa$

  $=4.91 atm$

Each gas in a gas mixture exerts its own pressure (partial pressure), which is independently of the pressure exerted by the other gases present. As a result, Dalton's law of partial pressures states that the total pressure placed by a mixture of gases equals the sum of the partial pressure of oxygen of the components.

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