The reaction of hydrogen and iodine to give hydrogen iodide has an equilibrium constant, Kc, of 56 at 435 °C.
- (a) What is the value of Kp?
- (b) Suppose you mix 0.045 mol of H2 and 0.045 mol of I2 in a 10.0-L flask at 425 °C. What is the total pressure of the mixture before and after equilibrium is achieved?
- (c) What is the partial pressure of each gas at equilibrium?
(a)
Interpretation:
The value of
Concept Introduction:
Equilibrium constant in terms of pressure
The activity of solid substance will not appear in equilibrium and numerically it is considered as one.
Answer to Problem 55GQ
The value of
Explanation of Solution
Given:
Using the equation
(b)
Interpretation:
The total pressure of the mixture before and after equilibrium has to be calculated.
Concept Introduction:
Equilibrium constant in terms of pressure
The activity of solid substance will not appear in equilibrium and numerically it is considered as one.
Answer to Problem 55GQ
The total pressure of the mixture before equilibrium and after equilibrium is
Explanation of Solution
Given:
From the reaction
Total pressure can be calculated using ideal gas equation
Total pressure of the mixture is
The total pressure before and after equilibrium will be the same since the amount of gas has not changed.
(c)
Interpretation:
The partial pressure of each gas in the mixture has to be calculated.
Concept Introduction:
Equilibrium constant in terms of pressure
The activity of solid substance will not appear in equilibrium and numerically it is considered as one.
Answer to Problem 55GQ
The partial pressures of each gas in the mixture is
Explanation of Solution
Given that initially
For the reaction
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