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Standard XII

Chemistry

Iron II Chloride

Nitric oxide ...

Question

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 constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate equilibrium amount of NO and Br₂.

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Solution

The given reaction is:

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 mol of Br, or

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

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Similar questions

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 constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate equilibrium amount of NO and Br₂.

Q. Nitric oxide reacts with bromine and gives nitrosyl-bromide as per reaction given below:

2 N O_{(g)} + B r_{2 (g)} ⇌ 2 N O B r_{(g)}

When

0.087

mole of

N O

and

0.0437

mole of

B r_{2}

are mixed is a closed container at constant temperature,

0.0518

mole of

N O B r

is obtained at equilibrium. Calculate the equilibrium amount of nitric oxide and bromine.

Q. When 0.087 mol of NO and 0.0437 mol of

B r_{2}

are mixed in a closed container at constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. The equilibrium amount of NO and

B r_{2}

are:

2 N O B r (g) ⇌ 2 N O (g) + {B r}_{2} (g)

. At equilibrium if nitrosyl bromide (

N O B r

) is

40

% dissociated at certain temp. and a total pressure of

0.30 a t m

K_{p}

for the reaction

2 N O (g) + {B r}_{2} (g) ⇌ 2 N O B r (g)

is:

N O

and

B r_{2}

at initial partial pressures of 98.4 and 41.3

torr

, respectively, were allowed to react at

300 K

. At equilibrium the total pressure was

110.5 torr

. Calculate the value of the equilibrium constant (

K p

) at

300 K

, for the reaction

2 N O (g) + B r_{2} (g) ⇌ 2 N O B r (g) .

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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 constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate equilibrium amount of NO and Br2.

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 constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. Calculate equilibrium amount of NO and Br₂.