Law of Mass Action
Chemistry ⇒ Chemical Kinetics and Equilibrium
Law of Mass Action starts at 11 and continues till grade 12.
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Describe how the Law of Mass Action is used to derive the equilibrium constant expression for a general reaction.
Describe the difference between Kc and Kp in the context of the Law of Mass Action.
Describe the role of stoichiometric coefficients in the Law of Mass Action.
Explain why pure solids and pure liquids are not included in the equilibrium constant expression derived from the Law of Mass Action.
Explain why the Law of Mass Action does not apply to reactions in non-ideal solutions.
Explain why the Law of Mass Action is important in chemical equilibrium studies.
Explain why the Law of Mass Action is not valid for very concentrated solutions.
For the reaction 2A + B ⇌ 3C, write the equilibrium constant expression.
For the reaction 2A ⇌ B + C, if the equilibrium concentrations are [A] = 0.2 M, [B] = 0.1 M, and [C] = 0.1 M, calculate Kc.
For the reaction 2NO2(g) ⇌ N2O4(g), if Kc = 4.0 at a certain temperature, and [NO2] = 0.5 M, calculate [N2O4] at equilibrium.
For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), write the equilibrium constant expression in terms of concentrations.
For the reaction 2X ⇌ Y + Z, if Kc = 0.5 and [X] = 0.4 M, [Y] = 0.1 M, calculate [Z] at equilibrium.
For the reaction A + B ⇌ C, if the initial concentrations are [A] = 1.0 M, [B] = 1.0 M, and at equilibrium [C] = 0.6 M, calculate Kc.
For the reaction A ⇌ B, if Kc = 2.0 and [A] = 0.5 M at equilibrium, what is [B]?
For the reaction aA + bB ⇌ cC + dD, write the expression for the equilibrium constant (Kc) according to the Law of Mass Action.
For the reaction aA + bB ⇌ cC, if the equilibrium concentrations are [A] = 1.0 M, [B] = 2.0 M, [C] = 3.0 M, a = 1, b = 2, c = 1, calculate Kc.
For the reaction H2(g) + I2(g) ⇌ 2HI(g), if [H2] = 0.5 M, [I2] = 0.5 M, and [HI] = 1.0 M at equilibrium, calculate Kc.
If the equilibrium constant (Kc) for a reaction is very large, what does it indicate about the position of equilibrium?
State the Law of Mass Action.
What is the effect of increasing the concentration of a reactant on the position of equilibrium, according to the Law of Mass Action?
