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# Nitric Oxide Reacts with Br2 And Gives Nitrosyl Bromide as per Reaction Given Below: When 0.087 Mol of No and 0.0437 Mol of Br2 Are Mixed in a Closed Container at the Constant Temperature, 0.0518 Mol of Nobr is Obtained at Equilibrium. Calculate Equilibrium Amount of No and Br2 . - CBSE (Science) Class 11 - Chemistry

ConceptLaw of Chemical Equilibrium and Equilibrium Constant

#### Question

Nitric oxide reacts with Br2 and gives nitrosyl bromide as per reaction given below:

2NO (g) + Br2 (g) ⇌ 2NOBr (g)

When 0.087 mol of NO and 0.0437 mol of Br2 are mixed in a closed container at the constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate equilibrium amount of NO and Br2 .

#### Solution 1

The given reaction is:

2NO_(g) + Br_(2(g)) ↔ 2NOBr_(g)

2mol        1mol           2mol

Now, 2 mol of NOBr are formed from 2 mol of NO. Therefore, 0.0518 mol of NOBr are formed from 0.0518 mol of NO.

Again, 2 mol of NOBr are formed from 1 mol of Br.

Therefore, 0.0518 mol of NOBr are formed from 0.0518/2 mol of Br, ot

0.0259 mol of NO.

The amount of NO and Br present initially is as follows:

[NO] = 0.087 mol [Br2] = 0.0437 mol

Therefore, the amount of NO present at equilibrium is:

[NO] = 0.087 – 0.0518

= 0.0352 mol

And, the amount of Br present at equilibrium is:

[Br2] = 0.0437 – 0.0259

= 0.0178 mol

#### Solution 2

The balanced chemical equation for the reaction is:

According to the equation, 2 moles of NO (g) react with 1 mole of Br(g) to form 2 moles of NOBr (g).

The composition of the equilibrium mixture can be calculated as follows:

No. of moles of NOBr (g) formed at equilibrium = 0.0518 mol (given)

No. of moles of NO (g) taking part in reaction = 0.0518 mol

No. of moles of NO (g) left at equilibrium = 0.087 – 0.0518 = 0.0352 mol

No. of moles of Br2 (g) taking part in reaction = 1/2 x 0.0518 = 0.0259 mol

No. of moles of Br2 (g) left at equilibrium = 0.0437 – 0.0259 = 0.0178 mol

The initial molar concentration and equilibrium molar concentration of different species may be represented as:
2NO (g) + Br2(g) ——————> 2NOBr(g)

Initial moles 0.087 0.0437 0

Moles at eqm. point: 0.0352 0.0178 0.0518

Is there an error in this question or solution?

#### APPEARS IN

Solution Nitric Oxide Reacts with Br2 And Gives Nitrosyl Bromide as per Reaction Given Below: When 0.087 Mol of No and 0.0437 Mol of Br2 Are Mixed in a Closed Container at the Constant Temperature, 0.0518 Mol of Nobr is Obtained at Equilibrium. Calculate Equilibrium Amount of No and Br2 . Concept: Law of Chemical Equilibrium and Equilibrium Constant.
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