At a given temperature, 4.92 atm of Cl2 and 4.65 atm of Br2 are mixed and allowed to come to equilibrium. The equilibrium pressure of BrCl is found to be 1.597 atm. Calculate Kp for the reaction at this temperature. Cl2(g) + Br2(g) <=> 2 BrCl(g). Give answer to 2 decimal places.

Kp = 0.16

Explanation:

Step 1: Data given

Initial pressure of Cl2 = 4.92 atm

Initial pressure of Br2 = 4.65 atm

The equilibrium pressure of BrCl is found to be 1.597 atm

Step 2: The balanced equation

Cl2(g) + Br2(g) ⇔ 2 BrCl(g

Step 3: The initial pressures

pCl2 = 4.92 atm

pBr2 = 4.65 atm

pBrCl = 0 atm

Step 4: The pressure at the equilibrium

For 1 mol Cl2 we need 1 mol Br2 to produce 2 moles BrCl

pCl2 = 4.92 - X atm

pBr2 = 4.65 - Xatm

pBrCl = 2X atm = 1.597 atm

X = 1.597/2 = 0.7985 atm

pCl2 = 4.92 - X atm = 4.92 - 0.7985 = 4.1215 atm

pBr2 = 4.65 - Xatm = 3.8515 atm

Step 5: Calculate Kp

Kp = (BrCl)² / (Cl2)*(Br2)

Kp = 1.597² / (4.1215*3.8515)

Kp = 0.16

i wish i could but this one is weird give me abc and i can solve it.