A sample of HI(g) is placed in flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI(g) is 0.04 atm. What of KP for the given equilibrium? 2HI(g)⇌H2(g)+I2(g) :
6
16
4
2
A
4
B
2
C
6
D
16
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Solution
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The equilibrium reaction is shown below. 2HI(g)⇌H2(g)+I2(g)
HI
H2
I2
Initial
0.2
0
0
Change
-2x
x
x
Equilibrium
0.2-2x
x
x
But the equilibrium pressure of HI is 0.04 atm. 0.2−2x=0.04 Hence, 2x=0.2−0.04=0.16 or x=0.08. The expression for the equilibrium constant is KP=PH2PI2P2HI=0.08×0.080.042=4.
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Q1
A sample of HI(g) is placed in flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI(g) is 0.04 atm. What of KP for the given equilibrium? 2HI(g)⇌H2(g)+I2(g) :
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Q2
A sample of HI(g) is placed in a flask at a pressure of 0.2 atm. At equilibrium partial pressure of HI(g) is 0.04 atm. What is Kp for the given equilibrium?
Given reaction is : 2HI(g)⇌H2(g)+I2(g)
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A sample of HI(g) is placed in flask at a pressure of 0.2 atm. At equilibrium the partial pressure of HI(g) is 0.04 atm. What is Kp for the given equilibrium?