Reactivity 2.3.2—The equilibrium law describes how the equilibrium constant, K, can be determined from the stoichiometry of a reaction. Deduce the equilibrium constant expression from an equation for a homogeneous reaction.

K_c for 2N₂O (g) $\rightleftharpoons$ 2N₂ (g) + O₂ (g) is 7.3 × 10³⁴.

What is K_c for the following reaction, at the same temperature?

N₂ (g) + $\frac{1}{2}$O₂ (g) $\rightleftharpoons$ N₂O (g)

A. 7.3 × 10³⁴

B. $\frac{1}{\sqrt{7.3\times {10}^{34}}}$

C. $\frac{1}{7.3\times {10}^{34}}$

D. $\frac{1}{2\times 7.3\times {10}^{34}}$

K_c for 2N₂O (g) $\rightleftharpoons$ 2N₂ (g) + O₂ (g) is 7.3 × 10³⁴.

What is K_c for the following reaction, at the same temperature?

N₂ (g) + $\frac{1}{2}$O₂ (g) $\rightleftharpoons$ N₂O (g)

A. 7.3 × 10³⁴

B. $\frac{1}{\sqrt{7.3\times {10}^{34}}}$

C. $\frac{1}{7.3\times {10}^{34}}$

D. $\frac{1}{2\times 7.3\times {10}^{34}}$

K_c for 2N₂O (g) $\rightleftharpoons$ 2N₂ (g) + O₂ (g) is 7.3 × 10³⁴.

What is K_c for the following reaction, at the same temperature?

N₂ (g) + $\frac{1}{2}$O₂ (g) $\rightleftharpoons$ N₂O (g)

A. 7.3 × 10³⁴

B. $\frac{1}{\sqrt{7.3\times {10}^{34}}}$

C. $\frac{1}{7.3\times {10}^{34}}$

D. $\frac{1}{2\times 7.3\times {10}^{34}}$

K_c for 2N₂O (g) $\rightleftharpoons$ 2N₂ (g) + O₂ (g) is 7.3 × 10³⁴.

What is K_c for the following reaction, at the same temperature?

N₂ (g) + $\frac{1}{2}$O₂ (g) $\rightleftharpoons$ N₂O (g)

A. 7.3 × 10³⁴

B. $\frac{1}{\sqrt{7.3\times {10}^{34}}}$

C. $\frac{1}{7.3\times {10}^{34}}$

D. $\frac{1}{2\times 7.3\times {10}^{34}}$

What is the equilibrium constant expression for the following equation?

2NO₂ (g) + F₂ (g) $\rightleftharpoons$ 2NO₂F (g)

A. $\frac{2[\text{N}{\text{O}}_2\text{F]}}{2[\text{N}{\text{O}}_2]+[{\text{F}}_2]}$

B. $\frac{2[\text{N}{\text{O}}_2\text{F]}}{2[\text{N}{\text{O}}_2][{\text{F}}_2]}$

C. $\frac{{[\text{N}{\text{O}}_2\text{]}}^2\text{[}{\text{F}}_2\text{]}}{{[\text{N}{\text{O}}_2\text{F}]}^2}$

D. $\frac{{[\text{N}{\text{O}}_2\text{F]}}^2}{{[\text{N}{\text{O}}_2]}^2[{\text{F}}_2]}$

What is the equilibrium constant expression for the following equation?

2NO₂ (g) + F₂ (g) $\rightleftharpoons$ 2NO₂F (g)

A. $\frac{2[\text{N}{\text{O}}_2\text{F]}}{2[\text{N}{\text{O}}_2]+[{\text{F}}_2]}$

B. $\frac{2[\text{N}{\text{O}}_2\text{F]}}{2[\text{N}{\text{O}}_2][{\text{F}}_2]}$

C. $\frac{{[\text{N}{\text{O}}_2\text{]}}^2\text{[}{\text{F}}_2\text{]}}{{[\text{N}{\text{O}}_2\text{F}]}^2}$

D. $\frac{{[\text{N}{\text{O}}_2\text{F]}}^2}{{[\text{N}{\text{O}}_2]}^2[{\text{F}}_2]}$

What is the equilibrium constant expression for the following equation?

2NO₂ (g) + F₂ (g) $\rightleftharpoons$ 2NO₂F (g)

A. $\frac{2[\text{N}{\text{O}}_2\text{F]}}{2[\text{N}{\text{O}}_2]+[{\text{F}}_2]}$

B. $\frac{2[\text{N}{\text{O}}_2\text{F]}}{2[\text{N}{\text{O}}_2][{\text{F}}_2]}$

C. $\frac{{[\text{N}{\text{O}}_2\text{]}}^2\text{[}{\text{F}}_2\text{]}}{{[\text{N}{\text{O}}_2\text{F}]}^2}$

D. $\frac{{[\text{N}{\text{O}}_2\text{F]}}^2}{{[\text{N}{\text{O}}_2]}^2[{\text{F}}_2]}$

What is the equilibrium constant expression for the following equation?

2NO₂ (g) + F₂ (g) $\rightleftharpoons$ 2NO₂F (g)

A. $\frac{2[\text{N}{\text{O}}_2\text{F]}}{2[\text{N}{\text{O}}_2]+[{\text{F}}_2]}$

B. $\frac{2[\text{N}{\text{O}}_2\text{F]}}{2[\text{N}{\text{O}}_2][{\text{F}}_2]}$

C. $\frac{{[\text{N}{\text{O}}_2\text{]}}^2\text{[}{\text{F}}_2\text{]}}{{[\text{N}{\text{O}}_2\text{F}]}^2}$

D. $\frac{{[\text{N}{\text{O}}_2\text{F]}}^2}{{[\text{N}{\text{O}}_2]}^2[{\text{F}}_2]}$

State the equilibrium constant expression, K_c, for the reaction above.

State the equilibrium constant expression, K_c, for the reaction above.

State the equilibrium constant expression, K_c, for the reaction above.

State the equilibrium constant expression, K_c, for the reaction above.

State the equilibrium constant expression, K_c, for the reaction above.

State the equilibrium constant expression, K_c, for the reaction above.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

Deduce the expression for the equilibrium constant, K_c, for this equation.

Deduce the expression for the equilibrium constant, K_c, for this equation.

Deduce the expression for the equilibrium constant, K_c, for this equation.

Deduce the expression for the equilibrium constant, K_c, for this equation.

Deduce the expression for the equilibrium constant, K_c, for this equation.

Deduce the expression for the equilibrium constant, K_c, for this equation.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.

State the equilibrium constant expression, K_c, for this reaction.