WorksheetsUnderstanding Chemical Equilibrium
Total questions: 10
Worksheet time: 5mins
What is chemical equilibrium?
Chemical equilibrium is when reactants are completely converted to products.
Chemical equilibrium is the point at which all reactions stop.
Chemical equilibrium is the state in which the concentrations of reactants and products remain constant because the forward and reverse reactions occur at the same rate.
Chemical equilibrium occurs only at high temperatures.
Describe the characteristics of a reversible reaction.
A reversible reaction does not reach equilibrium.
A reversible reaction can only proceed in one direction.
A reversible reaction can proceed in both directions, reaches dynamic equilibrium, and has constant concentrations of reactants and products.
A reversible reaction always produces more products than reactants.
What does Le Chatelier's principle state?
A system at equilibrium will always remain unchanged.
Le Chatelier's principle only applies to chemical reactions in gases.
Changes in pressure have no effect on equilibrium systems.
If a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to minimize the effect of that change.
How does temperature affect chemical equilibrium?
Temperature affects chemical equilibrium by shifting the position of equilibrium depending on whether the reaction is exothermic or endothermic.
Temperature has no effect on chemical equilibrium.
Increasing temperature always favors the formation of products.
Temperature only affects the rate of reaction, not equilibrium.
What is the equilibrium constant (K) and what does it signify?
The equilibrium constant (K) only applies to gases and not to liquids.
The equilibrium constant (K) is the sum of product and reactant concentrations.
The equilibrium constant (K) is a ratio of product concentrations to reactant concentrations at equilibrium.
The equilibrium constant (K) indicates the speed of a reaction.
Explain the difference between dynamic and static equilibrium.
Dynamic equilibrium involves ongoing processes at equal rates, whereas static equilibrium is a state of no movement or change.
Dynamic equilibrium is only found in chemical reactions.
Static equilibrium involves constant movement.
Dynamic equilibrium is a state of complete rest.
What role do catalysts play in chemical reactions at equilibrium?
Catalysts increase the rate of reaching equilibrium without changing the equilibrium position.
Catalysts slow down the rate of reactions at equilibrium.
Catalysts change the equilibrium position to favor products.
Catalysts are consumed in the reaction and do not affect equilibrium.
How can changes in concentration shift the position of equilibrium?
Decreasing concentration always shifts equilibrium to the left.
Increasing concentration always shifts equilibrium to the right.
Changes in concentration have no effect on equilibrium.
Changes in concentration shift the position of equilibrium by favoring the side of the reaction that reduces the change.
What is the significance of the reaction quotient (Q)?
Q determines the temperature of the reaction.
Q measures the concentration of reactants only.
The reaction quotient (Q) indicates the direction of a reaction relative to its equilibrium state.
Q is used to calculate the rate of a reaction.
Provide an example of a chemical reaction that reaches equilibrium.
N2(g) + 3H2(g) ⇌ 2NH3(g)
2H2(g) + O2(g) ⇌ 2H2O(g)
CaCO3(s) ⇌ CaO(s) + CO2(g)
C6H12O6 + 6O2 ⇌ 6CO2 + 6H2O
