CameraIcon

SearchIcon

MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Ideal Gas Equation

A vessel of v...

Question

A vessel of volume 5 litres contains 1.4 g of $N_{2}$ and 0.4 g of He at 1500 K. If 30% of the nitrogen molecules are dissociated into atoms then find the gas pressure.

Open in App

Solution

After dissolution, total moles will be $0.7 n + 2 (0.3) n = 1.3 n$ where n is initial moles of nitrogen. Hence,

$P (5 X 10^{- 3}) = (\frac{0.4}{4} + 1.3 \frac{1.4}{28}) (8.314) (1500)$

$P = \frac{0.165 X 8.314 X 1500}{5 X 10^{- 3}} = 4.1 X 10^{5} P a$

Answer is $4.1 X 10^{5} P a$

Suggest Corrections

thumbs-up

0

Similar questions

Q. A vessel having a volume of

5

litres contains

1.4 g

of nitrogen at a temperature of

1800 K

. The pressure of the gas if

30 %

of its molecules are dissociated into atoms at this temperature is:

Q. A vessel of volume

5

1.4 g

of nitrogen at a temperature

1800 K

. The pressure of the gas if

30

% of its molecules are dissociated into atoms at this temperature is :

Q. A vessel of volume 5L contains 1.4g of nitrogen at a temperature 1800K .The pressure of the gas if 30% of its molecules are dissociated into atoms at this temperature is

Q. A vessel having a volume of 5 litres contains

1.4 g

of nitrogen at a temperature of

1800 K

. The pressure of the gas if 30% of its molecules are dissociated into atoms at this temperature is:

Q. A 5 L vessel contains 1.4 g of nitrogen gas

N_{2}

. When heated to 1800 K, 30% of molecules are dissociated into atoms. Calculate the pressure of the gas at 1800 K. [Mol. mass of

N_{2} = 28 m o l^{- 1}

, R = 0.0821 L atm

K^{- 1} m o l^{- 1}

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

Adaptive Q18 hint

PHYSICS

Watch in App

explore_more_icon

Explore more

Ideal Gas Equation

Standard X Physics

Join BYJU'S Learning Program

CrossIcon