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
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