Question

A neon-dioxygen mixture contains 70.6 g dioxygen and 167.5 g neon. If pressure of the mixture of gases in the cylinder is 25 bar. What is the partial pressure of dioxygen and neon in the mixture ?​ ​

Answer 1

Explanation:

The partial pressure of dioxygen = 25 bar − 19.7 bar = 5.3 bar ..here's the answer

Answer 2

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The mass of dioxygen is 70.6 g.

The molar mass of dioxygen is 32 g/mol.

The number of moles of dioxygen

$= \frac{70.6g}{32g/mol} = 2.21mol$

The mass of neon is 167.5 g.

The molar mass of neon is 20.2 g/mol.

The number of moles of neon

$= \frac{167.5g}{20.2g/mol} = 8.29mol$

The total number of moles of neon and dioxygen

$= 2.21 + 8.29 = 10.49$

The mole fraction of neon

$= \frac{8.29}{10.49} = 0.789$

Total pressure in the cylinder is 25 bar.

The partial pressure of neon 

$= 0.789 \times 25bar = 19.7bar$

The partial pressure of dioxygen

$25bar - 19.7bar = 5.3bar$