N₂(g) + O₂(g) 2NO(g) K_c = 4.8 × 10^-31
2NOBr(g)
2NO(g) + Br₂(g) K_c = 0.50
Given the above equilibrium constant data at 25 °C, what is the value of K_c at this temperature for the reaction
2NOBr(g)
N₂(g) + O₂(g) + Br₂(g) ?

Question

N₂(g) + O₂(g)

N<sub>2</sub>(g) + O<sub>2</sub>(g) <sub> </sub> 2NO(g) K<sub>c</sub> = 4.8 × 10<sup>-31</sup> 2NOBr(g) <sub> </sub> 2NO(g) + Br<sub>2</sub>(g) K<sub>c</sub> = 0.50 Given the above equilibrium constant data at 25 °C, what is the value of K<sub>c</sub> at this temperature for the reaction 2NOBr(g) <sub> </sub> N<sub>2</sub>(g) + O<sub>2</sub>(g) + Br<sub>2</sub>(g) ? A) 2.4 × 10<sup>-31</sup> B) 9.6 × 10<sup>-31</sup> C) 1.0 × 10<sup>30</sup> D) 4.2 × 10<sup>30</sup> E) none of the above

2NO(g) K_c = 4.8 × 10^-31
2NOBr(g)

2NO(g) + Br₂(g) K_c = 0.50
Given the above equilibrium constant data at 25 °C, what is the value of K_c at this temperature for the reaction
2NOBr(g)

N₂(g) + O₂(g) + Br₂(g) ?

Quizplus · Accepted Answer

The Answer of N₂(g) + O₂(g) 2NO(g) K_c = 4.8 × 10^-31 2NOBr(g) 2NO(g) + Br₂(g) K_c = 0.50 Given the above equilibrium constant data at 25 °C, what is the value of K_c at this temperature for the reaction 2NOBr(g) N₂(g) + O₂(g) + Br₂(g)?

N2(g) + O2(g) 2NO(g) Kc = 4

N₂(g) + O₂(g) 2NO(g) K_c = 4