a neon gas mixture contains 70.6 g of o2 and 168 g of neon. if the pressure of mixture of gases is 24 bar what is the pressure of o2 and neon.

Open in App

Solution

1. Partial pressure of a gas in a mixture = $m o l e f r a c t i o n o f g a s \times t o t a l p r e s s u r e = \frac{n u m b e r o f m o l e s o f g a s}{t o t a l m o l e s o f g a s e s i n t h e s y s t e m} \times t o t a l p r e s s u r e$

2.
(a) Number of moles of Neon = $\frac{G i v e n m a s s}{m o l a r m a s s} = \frac{168 g}{20.17 g / m o l} = 8.33 m o l e s$

(b) Number of moles of oxygen = $\frac{70.6 g}{32 g / m o l} = 2.20 m o l e s$

Total moles of gases in the system = 2.20 + 8.33 = 10.53moles

3.
(a) Partial pressure of Neon = $\frac{8.33}{10.53} \times 24 b a r = 18.98 b a r$

(b) Partial pressure of Oxygen gas = $\frac{2.20}{10.53} \times 24 = 5.01 b a r$

Suggest Corrections

Similar questions

A neon dioxygen mixture contains 70.6 gram dioxygen and 167.5 gram 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 ?

Q. A neon-dioxygen mixture contains

70.6 g

dioxygen and

167.5 g

neon. If the pressure of the mixture of gases in the cylinder is

25

bar. What is the partial pressure of dioxygen and neon in the mixture?

Q. A neon-dioxygen mixture contains

70.6 g

dioxygen and

167.5 g

neon. If the pressure of the mixture of gases in the cylinder is 25 bar, what is the partial pressure of dioxygen and neon in the mixture?

A closed vessel contains a mixture of two gases Neon & Argon the total mass of mixture is 28 gm.The partial pressure due to Argon and neon are 4atm and 12atm respectively.The mass of individual gases in vessel is $(M_{n e o n} = 20, M_{a r g o n} = 40, R = 8.3 J / m o l - k)$

Q. A mixture of

H_{2}

and

O_{2}

gases in a cylinder contains

10 g H_{2}

and

64 g

O_{2}

. If the total pressure of the mixture of the gases in the cylinder is

35 bar

, the partial pressure of

H_{2}

gas is

Join BYJU'S Learning Program