Question

The equilibrium constant for the gas phase reaction N2 (g) + O2 (g) ⇌ 2NO (g) is Keq = 4.20 ⋅ 10-31 at 30 °C. At equilibrium, ________. The equilibrium constant for the gas phase reaction N2 (g) + O2 (g) 2NO (g) is Keq = 4.20 10-31 at 30 °C. At equilibrium, ________. products predominate reactants predominate roughly equal amounts of products and reactants are present only products are present only reactants are present

Answer 1

The equilibrium constant for the gas phase reaction N₂(g) + O₂(g) ⇌ 2NO(g) is Keq = 4.20x10⁻³¹ at 30 °C. At equilibrium, reactants predominate

Step-by-step explanation:

For the equilibrium

N₂(g) + O₂(g) ⇌ 2NO(g); Keq = 4.20x10⁻³¹

The formula is:

Keq =
`([NO]^2)/([N_(2)][O_(2)])`

As keq = 4.20x10⁻³¹

4.20x10⁻³¹ =
`([NO]^2)/([N_(2)][O_(2)])`

As keq <<< 1 mathematically [NO]²<<< [N₂][O₂]

That means, reactants predominate.

I hope it helps!

Answer 2

At equilibrium, reactants predominate.

Step-by-step explanation:

For every reaction, the equilibrium constant is defined as the ratio between the concentration of products and reactants. Thus, for the reaction N2 (g) + O2 (g) ⇌ 2NO the expression of its equilibrium constant is:

`Keq = ([NO]^(2))/([O_(2) ][N_(2)])`

Since the equilibrium constant is Keq = 4.20x10-31 the concentration of reactants O2 and N2 must be much higher than products to obtain such a small number as 4.20x10-31 at the equilibrium. Hence, at equilibrium reactants predominate.