Consider the equilibrium reaction shown below. B₂(g)
2B(g)
If the rate constants are: k_fwd = 7.00 × 10^-5 s^-1 and k_rev = 2.00 × 10^-5 L mol^-1 s^-1, what is the value of K_c under these conditions?

Question

Consider the equilibrium reaction shown below. B₂(g)

Consider the equilibrium reaction shown below. B<sub>2</sub>(g) <sub> </sub> 2B(g) If the rate constants are: k<sub>fwd</sub> = 7.00 × 10<sup>-5</sup> s<sup>-1</sup> and k<sub>rev</sub> = 2.00 × 10<sup>-5</sup> L mol<sup>-1</sup> s<sup>-1</sup>, what is the value of K<sub>c</sub> under these conditions? A) 1.75 × 10<sup>5</sup> B) 3.50 C) 0.286 D) 5.71 × 10<sup>-6</sup> E) 1.40 × 10<sup>-10</sup>

2B(g)
If the rate constants are: k_fwd = 7.00 × 10^-5 s^-1 and k_rev = 2.00 × 10^-5 L mol^-1 s^-1, what is the value of K_c under these conditions?

Quizplus · Accepted Answer

The Answer of Consider the equilibrium reaction shown below. B₂(g) 2B(g) If the rate constants are: k_fwd = 7.00 × 10^-5 s^-1 and k_rev = 2.00 × 10^-5 L mol^-1 s^-1, what is the value of K_c under these conditions?

Consider the Equilibrium Reaction Shown Below