At 1000 K, the equilibrium constant for the reaction 2NO (g) + Br2 (g) 2NOBr (g) is Kp = 0.013. Calculate Kp for the reverse reaction, 2NOBr (g) 2NO (g) + Br2 (g)

Kp for the reverse reaction is 76.9

Explanation:

Step 1: Kp at 1000 K = 0.013

Step 2: The balanced equation

2NO (g) + Br2 (g) ⇆ 2NOBr (g)

2NOBr (g) ⇆ 2NO (g) + Br2 (g)

Step 3: Calculate Kp

Kp for the reaction 2NO (g) + Br2 (g) ⇆ 2NOBr (g)

Kp = p(NOBr)²/(pBr2)*(pNO)²

Kp = 0.013

Kp for the reverse reaction 2NOBr (g) ⇆ 2NO (g) + Br2 (g)

Kp' = (pBr2)*(pNO)² /p(NOBr)²

Kp' = 1/Kp = 1/0.013 =  76.9

Kp for the reverse reaction is 76.9

bcde is the incorrect answer it is a

c) should be the answer.