Calculate the equilibrium constant for the chemical reaction, given the equilibrium concentrations of the reactants and products in the table. 2AB(aq)+4CD(aq)↽−−⇀2AD(aq)+2BD(aq)+4C(aq) 𝐾=

Question

AB	1.95 M
CD	2.17 M
AD	3.02 M
BD	4.61 M
C	2.52 M

Substance Equilibrium concentration

Answer 1

K=92.7

Let me know if this explanation helped!

K = ([C]^c[D]^d)/([B]^b[A]^a) for the reaction aA + bB ⇔ cC + dD

Substituting in the reaction 2AB (aq)+ 4CD (aq) ⇔ 2AD (aq)+ 2BD (aq)+ 4C (aq) , we get:

K = ([C]⁴[BD]²[AD]²)/([CD]⁴[AB]²)

Substituting in the values given in the table, we get:

K = (2.52⁴ * 4.61² * 3.02²)/(2.17⁴ * 1.95²)

K = 7816.6002/84.3156 = 92.71 = 92.7 (3 significant figures given in the table's values)

Answer 2

Where to start:

Identify the question:

Calculate the equilibrium constant (K_eq)

Identify the formula:

K_eq = {[product₁]ⁿ • [product₂]ⁿ } / {[reactant₁]ⁿ • [reactant₂]ⁿ}

n = coefficient of the compound from the balanced equation

Identify the products and reactants:

2AB(aq)+4CD(aq)↽−−⇀2AD(aq)+2BD(aq)+4C(aq)

Reactants ⇔ Products

*Only include (aq) compounds in the K_eq

Plug in coefficients as the exponent into the K_eq formula:

K_eq = {[AD]² • [BD]² • [C]⁴} / {[AB]² • [CD]⁴}

Plug in values from the chart:

K_eq = {[3.02]² • [4.61]² • [2.52]⁴} / {[1.95]² • [2.17]⁴}

K_eq = 92.71

ANSWER: K_eq = 92.71