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(3) 0.2 (4) 0.1 3. 1 mole of NO, and 2 moles of CO are enclosed in a one litre vessel to attain the following equilibrium NO, + CO — NO + CO. It was estimated that at the equilibrium, 25% of initial amount of CO is consumed. The equilibrium constant K, is (1) 1 (2) 1/2 (3) 1/4 Two moles of NH, gas are introduced into a (4) 1/3

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Q1

1 mole of

{N O}_{2}

and

2

moles of

C O

are enclosed in a one litre vessel to attain the following equilibrium

{N O}_{2} + C O ⇋ N O + {C O}_{2}

. It was estimated that at the equilibrium,

25 %

of initial amount of

C O

consumed. The equilibrium constant

K_{p}

is:

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Q2

1 mole of $N O_{2}$ and 2 moles of $C O$ are enclosed in a one litre vessel to attain the following equilibrium:

$N O_{2} + C O ⇌ N O + C O_{2}$

It was estimated that at the equilibrium, $25 %$ of the initial amount of $C O$ is consumed. The equilibrium constant $K_{p}$ is:

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Q3

1 mole of

N O_{2}

and 2 moles of

C O

are enclosed ina one litre vessel to attain the following equilibrium

N O_{2} + C O ⇋ N O + C O_{2}

. It was estimated that at the equilibrium, 25

%

of initial amount of

C O

isconsumed. The equilibrium constant

K_{0}

is

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Q4

At a certain temperature (T), the equilibrium constant

(K_{c})

is 1 for the reaction

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

If 2 moles of

N_{2},

4 moles of

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N H_{3}

and 3 moles of inert gas are introduced into a two litre rigid vessel at constant temperature T. It has been found that equilibrium concentration of

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and

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are equal then what is the equilibrium concentration of

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Q5

At

1000 K

, the equilibrium constant,

K_{c}

for the reaction,

C O (g) + {C l}_{2} (g) ⇌ C O {C l}_{2} (g)

,

is equal to

3.04

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1

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and

1

mole of

{C l}_{2}

are introduced into a

1

litre box at

1000 K

, what will be the final concentration of

C O {C l}_{2}

at equilibrium?

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