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steposvetlana [31]
3 years ago
12

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
Chemistry
2 answers:
pychu [463]3 years ago
5 0

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.

saveliy_v [14]3 years ago
3 0

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, <em>reactants predominate</em>

Explanation:

For the equilibrium

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

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, <em>reactants predominate. </em>

<em></em>

I hope it helps!

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