A sample of nitrosyl bromide (nobr) decomposes according to the equation 2nobr (g) ⇌2no (g) + br2 (g) an equilibrium mixture in a 5.00-l vessel at 100 ∘c contains 3.26 g of nobr, 3.06 g of no, and 8.15 g of br2. part a calculate kc.

Question

Regina Bradshaw

Chemistry

24 October, 10:05

A sample of nitrosyl bromide (nobr) decomposes according to the equation 2nobr (g) ⇌2no (g) + br2 (g) an equilibrium mixture in a 5.00-l vessel at 100 ∘c contains 3.26 g of nobr, 3.06 g of no, and 8.15 g of br2. part a calculate kc.

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Answers (1)

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Susie Q · Answer 1

Kc = 0.122.

Explanation:

We can calculate Kc from the relation: Kc = [NO]².[Br₂] / [NOBr]². Firstly, we convert the number of grams of each component to moles using (n = mass / molar mass). n of NOBr = (3.26 g / 109.8 g/mole) = 0.03 moles. n of NO = (3.06 g / 29.9 g/mole) = 0.102 moles. n of Br₂ = (8.15 g / 159.9 g/mole) = 0.051 moles. Then we can get the concentration of each component by dividing its no. of moles by the volume of the vessel (concentration = n / V). The concentration of NOBr = (0.03 mole / 5.00 L) = 6x10⁻³ mol/L. The concentration of NO = (0.102 mole / 5.00 L) = 2x10⁻² mol/L. The concentration of Br₂ = (0.051 mole / 5.00 L) = 1x10⁻² mol/L. Now, we can get Kc: Kc = [NO]².[Br₂] / [NOBr]² = (2x10⁻² mol/L) ². (1x10⁻² mol/L) / (6x10⁻³ mol/L) ² = 0.122.