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

Answer:

At equilibrium, reactants predominate.

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:

$Keq = \frac{[NO]^{2}}{[O_{2} ][N_{2}]}$

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.

Answer 2

Answer:

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

Explanation:

For the equilibrium

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

The formula is:

Keq = $\frac{[NO]^2}{[N_{2}][O_{2}]}$

As keq = 4.20x10⁻³¹

4.20x10⁻³¹ = $\frac{[NO]^2}{[N_{2}][O_{2}]}$

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

That means, reactants predominate.

I hope it helps!