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:
[tex]Keq = \frac{[NO]^{2}}{[O_{2} ][N_{2}]}[/tex]
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:
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 = [tex]\frac{[NO]^2}{[N_{2}][O_{2}]}[/tex]
As keq = 4.20x10⁻³¹
4.20x10⁻³¹ = [tex]\frac{[NO]^2}{[N_{2}][O_{2}]}[/tex]
As keq <<< 1 mathematically [NO]²<<< [N₂][O₂]
That means, reactants predominate.
I hope it helps!
