Very few chemical reactions go to completion. Instead, most reach a state called

Question

Very few chemical reactions go to completion. Instead, most reach a state called chemical equilibrium in which both products and reactants are present. The concentrations of reactants and products can be predicted using the equilibrium constant, Kc, which is a mathematical expression based on the chemical equation. For example, in the reaction

aA(aq)+bB(aq)cC(aq)+dD(aq)

where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is

Kc=[C]c[D]d[A]a[B]b

where [A], [B], [C], and [D] are the equilibrium concentrations. If the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, Qc, instead of the equilibrium constant, Kc.

Part A

A mixture initially contains A, B, and C in the following concentrations: [A]=0.600mol L1, [B]=1.25mol L1, and [C]=0.400mol L1. The following reaction occurs and equilibrium is established:

A(aq)+2B(aq)C(aq)

At equilibrium, [A]=0.450mol L1 and [C]=0.550mol L1. Calculate the value of the equilibrium constant, Kc .

Explanation / Answer

given data,

A(aq) + 2B(aq) C(aq)

Intial : 0.600 1.25 0

at equilibrium : 0.600-x 1.25-x x

but at equilibrium   [C]=0.550mol L1. = x= 0.55

the equilibrium constant, Kc . = [C] / [A] x  [B] 2

   = 0.55 / 0.45x(0.7)2

= 2.49433

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