
The equilibrium constant KP for the following reaction is 4.31 × 10−4 at 375°C:
In a certain experiment a student starts with 0.862 atm of N2 and 0.373 atm of H2 in a constant-volume vessel at 375°C. Calculate the partial pressures of all species when equilibrium is reached.

Interpretation:
Calculate the partial pressure values all species of reactant and product given the equilibrium reaction at
Concept Introduction:
Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.
Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.
Kp and Kc: This equilibrium constants of gaseous mixtures, these difference between the two constants is that Kc is defined by molar concentrations, whereas Kp is defined by the partial pressures of the gasses inside a closed system.
Answer to Problem 14.84QP
The reactant and product partial equilibrium pressure (Kp) values for the given
Explanation of Solution
To find: The equilibrium reaction should be identified given the statement.
Analyze the chemical equilibrium reaction.
The given equilibrium concentration reaction is the combined reaction is the product of the constants for this component reaction. This equilibrium reaction expression contains different conditions like solid phase into gases phase, so this process homogenous equilibrium the equilibrium constant can also be represented by Kp, were the Kp represents partial pressure. Then the each (reactant and product) molecule partial pressure
To find: Calculate the each partial pressure (Kp) values for given the statement of equilibrium reaction.
Calculate and analyze the (Kp) values at
Consider the given equilibrium reactions
The given ammonia formation reaction the respective reactant to give products all exists in the same phase and this equilibrium reaction expression contains single conditions like gases phase, the equilibrium constant can also be represented by Kp, were the “P” partial pressure. The each partial pressure values are Kp derived given equation at
The each of reactant and product partial pressure (Kp) values are derived given the ammonia
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Chapter 14 Solutions
Loose Leaf for Chemistry
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