Assume that the equilibrium constant for the following reaction is known.

2 NO₂(g) 2 NO(g) + O₂(g) K₁ = 7.4 x 10^-16 (at 25°C)

What is the correct value of the equilibrium constant for the opposite reaction?
2 NO(g) + O₂(g) 2 NO₂(g) K₂ = ?

Question

Assume that the equilibrium constant for the following reaction is known.

2 NO₂(g)

Assume that the equilibrium constant for the following reaction is known. 2 NO<sub>2</sub>(g) 2 NO(g) + O<sub>2</sub>(g) K<sub>1</sub> = 7.4 x 10<sup>-16</sup> (at 25°C) What is the correct value of the equilibrium constant for the opposite reaction? 2 NO(g) + O<sub>2</sub>(g) 2 NO<sub>2</sub>(g) K<sub>2</sub> = ? A) K<sub>2</sub> = K<sub>1</sub> = 7.4 x 10<sup>-16</sup> B) K<sub>2</sub> = 1/K<sub>1</sub> = 1.4 x 10<sup>15</sup> C) K<sub>2</sub> = K<sub>1</sub>(RT) = 1.8 x 10<sup>-14</sup> D) K<sub>2</sub> = K<sub>1</sub>(RT) <sup>-1</sup> = 3.0 x 10<sup>-17</sup> E) impossible to determine from this information

2 NO(g) + O₂(g) K₁ = 7.4 x 10^-16 (at 25°C)

What is the correct value of the equilibrium constant for the opposite reaction?
2 NO(g) + O₂(g)

2 NO₂(g) K₂ = ?

Quizplus · Accepted Answer

The Answer of Assume that the equilibrium constant for the following reaction is known. 2 NO₂(g) 2 NO(g) + O₂(g) K₁ = 7.4 x 10^-16 (at 25°C) What is the correct value of the equilibrium constant for the opposite reaction? 2 NO(g) + O₂(g) 2 NO₂(g) K₂ = ?

Assume That the Equilibrium Constant for the Following Reaction Is