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Liquids in Liquids

A vessel cont...

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A vessel contains 28 gm of N2 and 32 gm of O2, at temperature T=1800 K and pressure 2 atm. Find the pressure if N2 dissociate 30 % and O2 dissociate 50% if temperature remains constant (1) 2 atm (2) 1 atm (3) 2.8 atm (4) 1.4 atm

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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:

N_{2}

H_{2}

are placed in a closed container at a pressure of 4 atm. The pressure falls to 3 atm at the same temperature when the following equilibrium is attained.

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

. The equilibrium constant

K_{p}

for dissociation of

N H_{3}

1

N_{2}

3

H_{2}

are placed in a closed container at a pressure of

4

atm. The pressure falls to

3

atm at the same temperature when the equilibrium is attained

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {N H}_{3} (g)

. The equilibrium constant

K_{p}

for dissociation of

{N H}_{3}

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}

1

N_{2}

3

H_{2}

are placed in a closed container at a pressure of

4

atm. The pressure falls to

3

atm at the same temperature when the following equilibrium is attained:

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

The equilibrium constant

K_{p}

for dissociation of

N H_{3}

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