Chemical Equilibrium
Chemistry ⇒ Chemical Kinetics and Equilibrium
Chemical Equilibrium starts at 10 and continues till grade 12.
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A reaction at equilibrium has K_c = 1. What does this indicate about the concentrations of reactants and products?
A reaction has K_c = 0.01. Is the reaction product-favored or reactant-favored at equilibrium?
A reaction mixture at equilibrium contains 0.4 mol/L of D, 0.2 mol/L of E, and 0.1 mol/L of F for the reaction: D \rightleftharpoons E + F. Calculate K_c.
A reaction mixture contains 0.2 mol/L of A, 0.3 mol/L of B, and 0.5 mol/L of C at equilibrium for the reaction: A + B \rightleftharpoons C. Calculate the equilibrium constant K_c.
Describe what happens to the equilibrium position if the pressure is decreased for a reaction where the number of moles of gas is greater on the reactant side.
Describe what happens to the position of equilibrium if the concentration of a reactant is increased.
Describe what is meant by a homogeneous equilibrium.
Explain the effect of decreasing the temperature on the equilibrium position of an endothermic reaction.
Explain why equilibrium is described as a dynamic process.
Explain why solids and pure liquids are not included in the equilibrium constant expression.
For the reaction: 2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g), what will happen to the equilibrium position if the pressure is increased?
For the reaction: H_2(g) + I_2(g) \rightleftharpoons 2HI(g), what will happen to the equilibrium position if more HI is added?
For the reaction: N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g), write the expression for the equilibrium constant K_c.
State Le Chatelier’s Principle.
State two conditions necessary for a chemical equilibrium to be established.
What does it mean if K_c is much less than 1?
What is meant by chemical equilibrium?
What is the equilibrium constant (K_c)?
A sealed container contains the following equilibrium: CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g). Predict and explain the effect on the equilibrium position if the volume of the container is halved.
A student claims that at equilibrium, the concentrations of reactants and products must be equal. Is this statement correct? Explain your answer.
