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Standard XI

Chemistry

Derivation of Kp and Kc

In a reaction...

Question

In a reaction vessel of 2 litre capacity 3 moles of $N_{2}$ reacts with 2 moles of $O_{2}$ to produce 1 mole of NO according to following reaction-
$N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$ . What is the molar concentration of $N_{2}$ at equilibrium?

1.25

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1.5

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0.75

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Solution

The correct option is A 1.25
$\begin{matrix} N_{2} & + & O_{2} & ⇌ & 2 N O 3 & 2 & 0 3 - x & 2 - x & 2 x \end{matrix}$
$∵ 2 x = 1; x = 0.5$
$[N_{2}] = \frac{3 - 0.5}{2} = 1.25$

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Similar questions

Q. In a reaction vessel of 2 litre capacity 3 moles of

N_{2}

reacts with 2 moles of

O_{2}

to produce 1 mole of NO according to following reaction-

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

. What is the molar concentration of

N_{2}

at equilibrium?

Q. In a reaction vessel of 2 litre capacity 3 moles of

N_{2}

reacts with 2 moles of

O_{2}

to produce 1 mole of NO according to following reaction-

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

. What is the molar concentration of

N_{2}

at equilibrium?

Q. In a reaction vessel of 2 liter capacity 3 moles of

N_{2}

reacts with 2 moles of

O_{2}

to produce 1 mole of NO. What is the molar concentration of

N_{2}

at equilibirium ?

Q. The equilibrium

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

is estabilished in a reaction vessel of

2.5 L

capacity amount of

N_{2}

and

O_{2}

taken at the start were respectively

2

moles and

4

moles. Half a mole of nitrate been used up at equilibrium. The molar concentration of nitric oxide is

Q. The equilibrium

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

established in a reaction vessel of

2.5

L capacity. The amounts of

N_{2}

and

O_{2}

taken at the start were respectively

2

moles and

4

moles. Half a mole of nitrogen has been used up at equilibrium. The molar concentration of nitric oxide is :

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Derivation of Kp and Kc

Standard XI Chemistry

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In a reaction vessel of 2 litre capacity 3 moles of N2 reacts with 2 moles of O2 to produce 1 mole of NO according to following reaction- N2(g)+O2(g)⇌2NO(g). What is the molar concentration of N2 at equilibrium?

The correct option is A 1.25N2+O2⇌2NO3203−x2−x2x ∵ 2x=1;x=0.5 [N2]=3−0.52=1.25

In a reaction vessel of 2 litre capacity 3 moles of $N_{2}$ reacts with 2 moles of $O_{2}$ to produce 1 mole of NO according to following reaction-
$N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)$ . What is the molar concentration of $N_{2}$ at equilibrium?

The correct option is A 1.25
$\begin{matrix} N_{2} & + & O_{2} & ⇌ & 2 N O 3 & 2 & 0 3 - x & 2 - x & 2 x \end{matrix}$
$∵ 2 x = 1; x = 0.5$
$[N_{2}] = \frac{3 - 0.5}{2} = 1.25$