Question

Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached PNO=0.526atm, PBᵣ₂= 1.59 atm, and PNOBᵣ=7.68atm. Calculate Kp for the reaction: 2NOBᵣ(g)⇌2NO(g)+Bᵣ₂(g).

a) 0.035
b) 0.071
c) 0.108
d) 0.125

Answer 1

To calculate Kp for the reaction: 2NOBr(g) ⇒ 2NO(g) + Br2(g), we need to use the given equilibrium partial pressures of the gases. By denoting the change in the partial pressure of NO as 2x and the change in the partial pressure of Br2 as x, we can set up equations to find the equilibrium partial pressures. However, without enough information about these partial pressures, we cannot calculate the value of Kp for this reaction.

Step-by-step explanation:

To calculate Kp for the reaction: 2NOBr(g) ⇒ 2NO(g) + Br2(g), we need to use the equilibrium partial pressures of the gases. From the given information, P(NOBr) = 1.25 atm and P(Br2) = 8.5 x 10-5 atm. Let's denote the change in the partial pressure of NO as 2x, then the change in the partial pressure of Br2 is also x because 2 mol of NOBr reacts to form 1 mol of Br2. The equilibrium partial pressures of the gases can be calculated based on the initial pressures and the changes:

P(NO) = 1.25 + 2x

P(Br2) = 8.5 x 10-5 + x

Now, we can substitute these values into the expression for Kp:

Kp = (P(NO))² (P(Br2)) = [(1.25 + 2x)²][(8.5 x 10-5 + x)]

To find the equilibrium constant, we need to solve for x and substitute it back into the expression for Kp. Unfortunately, we don't have enough information to calculate the value of x and determine the equilibrium constant. Therefore, we cannot determine the value of Kp for this reaction.