Respuesta :
Answer: The equilibrium partial pressure of HCl is 7.20 atm
Explanation:
We are given:
Initial partial pressure of hydrogen gas = 4 atm
Initial partial pressure of chlorine gas = 6 atm
For the given chemical equation:
[tex]H_2(g)+Cl_2(g)\rightleftharpoons 2HCl(g)[/tex]
Initial: 4 6
At eqllm: 4-x 6-x 2x
The expression of [tex]K_p[/tex] for above equation follows:
[tex]K_p=\frac{(p_{HCl})^2}{p_{H_2}\times p_{Cl_2}}[/tex]
We are given:
[tex]K_p=54[/tex]
Putting values in above equation, we get:
[tex]54=\frac{(2x)^2}{(4-x)\times (6-x)}\\\\x=3.6,7.2[/tex]
Neglecting the value of x = 7.2 because equilibrium partial pressure cannot be greater than initial partial pressure
So, equilibrium partial pressure of HCl = [tex]2x=(2\times 3.6)=7.20atm[/tex]
Hence, the equilibrium partial pressure of HCl is 7.20 atm
Answer:
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
