7.9. Nitric oxide reacts with Br2and gives nitrosyl bromide as per reaction given below: 2NO (g) + Br2 (g) ?? 2NOBr (g) When 0.087 mole of NO and 0.0437 mole of Br2 are mixed in a closed container at constant temperature, 0.0518 mole of NOBr is obtained at equilibrium. Determine the compositions of the equilibrium mixture.

According to the equation, 2 moles of NO (g) react with 1 mole of Br2 (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 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) NO Br2 NOBr Initial moles 0.087 0.0437 0 Change -2x -x 2x Moles at equilibrium 0.0352 0.0178 0.0518

7.9. Nitric oxide reacts with Br₂and gives nitrosyl bromide as per reaction given below:

2NO (g) + Br₂ (g) ?? 2NOBr (g)
When 0.087 mole of NO and 0.0437 mole of Br₂ are mixed in a closed container at constant temperature, 0.0518 mole of NOBr is obtained at equilibrium. Determine the compositions of the equilibrium mixture.

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Vishal Baghel | Contributor-Level 10

9 months ago

According to the equation, 2 moles of NO (g) react with 1 mole of Br₂ (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
No. of moles of NO (g) taking part in reaction = 0.0518 mol
No.