In the reaction below, 4 atm of H2 and 6 atm of Cl2 were placed into a 1.00 L flask and allowed to react: H2(g) + Cl2(g) <=> 2 HCl(g) Given that Kp at 700 K = 54, calculate the equilibrium pressure of HCl. Give your answer to 2 decimal places.

The partial pressure of HCl is 7.2 atm

Explanation:

Step 1: Data given

Pressure of H2 = 4.0 atm

Pressure of Cl2 = 6.0 atm

Volume 1.00 L

Step 2: The balanced equation

H2(g) + Cl2(g) <=> 2 HCl(g)

Step 3: The initial pressure

H2: 4.0 atm

Cl2: 6.0 atm

HCl: 0 atm

Step 4: Calculate pressure at the equilibrium

For 1 mol H2 there will react 1 mol Cl2 to produce 2 moles HCl

H2: (4.0 -X)atm

Cl2: (6.0-X)atm

HCl: 2X atm

Kp = 54 = (pHCl)² / (pH2)(pCl2)

54 = (4X)² / (4.0 - X)(6.0-X)

X = 3.6

The partial pressure of HCl = 2X atm

2X = 2*3.6 atm = 7.2 atm

The partial pressure of HCl is 7.2 atm

you gotta add the following molecules so we can give u an answer

explanation: