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Assume That the Equilibrium Constant for the Following Reaction Is

Question 20

Multiple Choice

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) 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 NO2(g)   K2 = ?


A) K2 = K1 = 7.4 x 10-16
B) K2 = 1/K1 = 1.4 x 1015
C) K2 = K1(RT) = 1.8 x 10-14
D) K2 = K1(RT) -1 = 3.0 x 10-17
E) impossible to determine from this information

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