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(a)
Interpretation:
The equilibrium position should be draw and analyzed the given equilibrium reactions.
Concept Introduction:
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.
Equilibrium concentration: If (Kc) and the initial concentration for a reaction and calculate for both equilibrium concentration and example using (ICE) chart and equilibrium constant and derived changes in respective reactants and products.
To Identify: Given the statements of reactions (a-c) equilibrium positions draw and analyzed.
(b)
Interpretation:
The equilibrium position should be draw and analyzed the given equilibrium reactions.
Concept Introduction:
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.
Homogeneous equilibrium: A homogeneous equilibrium involved has a everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.
Equilibrium concentration: If (Kc) and the initial concentration for a reaction and calculate for both equilibrium concentration and example using (ICE) chart and equilibrium constant and derived changes in respective reactants and products.
Given the statements of reactions (a-c) equilibrium positions draw and analyzed.
(c)
Interpretation:
The equilibrium position should be draw and analyzed the given equilibrium reactions.
Concept Introduction:
Chemical equilibrium reaction: The term applied to reversible chemical reactions. It is the point at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium is achieved; the concentrations of reactant and products become constant.
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.
Homogeneous equilibrium: A homogeneous equilibrium involved has a everything present in the same phase and same conditions, for example reactions where everything is a gas, or everything is present in the same solution.
Equilibrium concentration: If (Kc) and the initial concentration for a reaction and calculate for both equilibrium concentration and example using (ICE) chart and equilibrium constant and derived changes in respective reactants and products.
To Identify: Given the statements of reactions (a-c) equilibrium positions draw and analyzed.
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Chapter 15 Solutions
General Chemistry
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