1. A neon-dioxygen mixture contains 70.6 g
dioxygen and 167.5g neon. If pressure of
the mixture of the gases in the cylinder
is 25 bar. What is the partial pressure of
dioxygen and neon in the mixture?
Answers
Answer:
The mass of dioxygen is 70.6 g.
The molar mass of dioxygen is 32 g/mol.
The number of moles of dioxygen
=
32 g/mol
70.6 g
= 2.21 mol
The mass of neon is 167.5 g.
The molar mass of neon is 20.2 g/mol.
The number of moles of neon
=
20.2 g/mol
167.5 g
= 8.29 mol
The total number of moles of neon and dioxygen = 2.21 + 8.29= 10.49
The mole fraction of neon =
10.49
8.29
= 0.789
Total pressure in the cylinder is 25 bar.
The partial pressure of neon = 0.789 × 25 bar= 19.7 bar
The partial pressure of dioxygen = 25 bar − 19.7 bar = 5.3 bar The mass of dioxygen is 70.6 g.
The molar mass of dioxygen is 32 g/mol.
The number of moles of dioxygen
=
32 g/mol
70.6 g
= 2.21 mol
The mass of neon is 167.5 g.
The molar mass of neon is 20.2 g/mol.
The number of moles of neon
=
20.2 g/mol
167.5 g
= 8.29 mol
The total number of moles of neon and dioxygen = 2.21 + 8.29= 10.49
The mole fraction of neon =
10.49
8.29
= 0.789
Total pressure in the cylinder is 25 bar.
The partial pressure of neon = 0.789 × 25 bar= 19.7 bar
The partial pressure of dioxygen = 25 bar − 19.7 bar = 5.3 bar