Question

Given the reaction: A + B <--> C + D

The concentrations at equilibrium are [A] = 1 M, [B] = 1 M, [C] = 2 M, and [D] = 2 M. What is the value of the equilibrium constant (K)?
Group of answer choices

A. 4.0

B. 2.0

C. 1.0

D. 0.25

Answer 1

A.) 4.0

Step-by-step explanation:

The general equilibrium expression looks like this:

`K = ([C]^(c) [D]^(d) )/([A]^(a) [B]^(b) )`

In this expression,

-----> K = equilibrium constant

-----> uppercase letters = molarity

-----> lowercase letters = balanced equation coefficients

In this case, the molarity's do not need to be raised to any numbers because the coefficients in the balanced equation are all 1. You can find the constant by plugging the given molarities into the equation and simplifying.

`K = ([C]^(c) [D]^(d) )/([A]^(a) [B]^(b) )` <----- Equilibrium expression

`K = ([2 M] [2 M])/([1 M] [1 M] )` <----- Insert molarities

`K = (4)/(1 )` <----- Multiply

`K = 4` <----- Divide