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The following reaction has a value of Kc = 3.07 x 10-4 at 25o C. A reaction is studied with the initial concentrations of [NO] = 1.58 x 10-2 M, [Br2] = 1.29 x 10-2 M, and [NOBr] = 7.13 x 10-2 M
2 NOBr (g) <_____> 2 NO (g) + Br2 (g)Choose the one correct statement from the following: (A) Qc = 1.58 x 104 and the concentration of NOBr will decrease.(B) Qc = 6.33 x 10-4 and the concentration of NOBr will increase.(C) Qc = 2.85 x 10-3 and the concentration of NOBr will increase.
(D) Qc = 2.85 x 10-3 and the concentration of NOBr will decrease.

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Answer:

Qc = 6.33 x 10-4 and the concentration of NOBr will increase

Explanation:

2 NOBr (g) →  2NO (g) + Br₂(g)

Qc = Reaction quotient. It tells us the quantity of products and reactants during the reaction at a particular point in time, other than equilibrium.

The expression for Qc is the same for Kc

Qc = ([NO]² . [Br]) / [NOBr]²

Qc = ((1.58x10⁻²)² . 1.29x10⁻²) / (7.13x10⁻²)²

Qc = 6.33x10⁻⁴

You have to compare Qc to Kc to analyse the reaction:

Qc < Kc → Some reagents have not generated products yet.

Reaction tends to Products

Qc > Kc → Reaction tends to Reactants.

Reactants concentration must be increased to make more products

Qc = Kc →  Equilibrium

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