Question

Consider the reaction below. H2(g) + CO2(g) mc013-1.jpg H2O(g) + CO(g) At equilibrium at 600 K, the following are true. [CO2] = 9.5 x 10-4 M [H2] = 4.5 x 10-2 M [H2O] = 4.6 x 10-3 M [CO] = 4.6 x 10-3 M What is the value of the equilibrium constant for this reaction in correct scientific notation? 4.9 x 10-3 4.9 x 10-2 4.9 x 10-1 4.9 x 103

Answer 1

The correct answer is C

Answer 2

Ans: c) 4.9 *10-1

Given:

Concentrations of the reactants and products-

[CO2] = 9.5 x 10-4 M

[H2] = 4.5 x 10-2 M

[H2O] = 4.6 x 10-3 M

[CO] = 4.6 x 10-3 M

To determine:

The equilibrium constant K

Step-by-step explanation:

The given reaction is:

H2(g) + CO2(g) ↔ H2O(g) + CO(g)

The equilibrium constant is given as:

`K = ([H2O]*[CO])/([H2]*[CO2]) \\\\K = (4.6 x 10^(-3)  M * 4.6 x 10^(-3)  M)/(4.5 x 10^(-2) 10-2 M*9.5 x 10^(-4)  M) \\\\K = 0.4949 = 4.9 *10^(-1)`