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WorksheetsChemical Equilibrium Basics
Total questions: 15
Worksheet time: 8mins
What is the main difference between heterogeneous and homogeneous equilibrium?
Heterogeneous equilibrium involves only reactants; homogeneous equilibrium involves only products.
Heterogeneous equilibrium occurs in closed systems; homogeneous equilibrium occurs in open systems.
In heterogeneous equilibrium, reactants and products are in different phases; in homogeneous equilibrium, all reactants and products are in the same phase.
In heterogeneous equilibrium, reactants and products are in the same phase; in homogeneous equilibrium, all reactants and products are in different phases.
Give an example of a heterogeneous equilibrium reaction.
The reaction: CaCO3(s) + CO2(g) ⇌ CaO(s) + CO2(g)
The reaction: H2(g) + I2(g) ⇌ 2HI(g)
The reaction: N2(g) + 3H2(g) ⇌ 2NH3(g)
The reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g)
Explain why the equilibrium constant for a heterogeneous reaction may include only the concentrations of gases or liquids.
The concentrations of solids are highly variable and affect the equilibrium position significantly.
The concentrations of solids are constant and do not affect the equilibrium position.
The concentrations of gases are not involved in the reaction.
The equilibrium constant is not affected by the nature of the substances involved.
How does the presence of a catalyst affect the position of equilibrium in a homogeneous reaction?
A catalyst shifts the equilibrium to the left in a homogeneous reaction.
A catalyst increases the concentration of reactants at equilibrium in a homogeneous reaction.
A catalyst does not affect the position of equilibrium in a homogeneous reaction.
A catalyst decreases the rate of the reaction in a homogeneous reaction.
Discuss the role of temperature in shifting the equilibrium in a heterogeneous system.
Increasing temperature always shifts the equilibrium towards the reactants
Temperature has no impact on equilibrium in a heterogeneous system
Temperature affects the equilibrium by changing the rate of reactions and shifting it towards the endothermic or exothermic direction.
Temperature only affects homogeneous systems, not heterogeneous ones
What is the effect of pressure changes on a heterogeneous equilibrium?
Pressure changes increase the rate of reaction in a heterogeneous equilibrium.
Pressure changes shift the equilibrium towards the side with fewer moles of gas.
Pressure changes cause the equilibrium to completely shift to one side.
Pressure changes do not affect a heterogeneous equilibrium.
Describe how Le Chatelier's Principle applies to a homogeneous equilibrium.
Le Chatelier's Principle does not affect homogeneous equilibrium
In a homogeneous equilibrium, Le Chatelier's Principle always leads to a decrease in reactants
In a homogeneous equilibrium, Le Chatelier's Principle applies by shifting the equilibrium position in response to changes in concentration, pressure, or temperature.
Homogeneous equilibrium is not influenced by concentration, pressure, or temperature changes
Why is it important to consider the phase of reactants and products in a heterogeneous equilibrium?
Considering the phase of reactants and products is important in a heterogeneous equilibrium because it affects the equilibrium constant expression.
Phase changes do not influence the position of equilibrium
The phase of reactants and products has no impact on equilibrium
Equilibrium constants are not affected by the phase of substances
Compare and contrast the characteristics of a homogeneous and heterogeneous equilibrium.
Homogeneous equilibrium occurs at high temperatures, while heterogeneous equilibrium occurs at low temperatures.
Homogeneous equilibrium involves only reactants, while heterogeneous equilibrium involves only products.
Homogeneous equilibrium is reversible, while heterogeneous equilibrium is irreversible.
Homogeneous equilibrium involves all reactants and products in the same phase, while heterogeneous equilibrium involves reactants and products in different phases.
Explain the concept of dynamic equilibrium in a chemical reaction.
Dynamic equilibrium is achieved when the rate of the forward reaction equals the rate of the reverse reaction, maintaining constant concentrations of reactants and products.
Dynamic equilibrium occurs when the reaction stops completely.
Dynamic equilibrium is only achieved in irreversible reactions.
Dynamic equilibrium means the reaction proceeds in only one direction.
How does the rate of the forward reaction compare to the rate of the reverse reaction at equilibrium?
The rate of the forward reaction is equal to the rate of the reverse reaction at equilibrium.
The rate of the forward reaction is zero at equilibrium.
The rate of the forward reaction is greater than the rate of the reverse reaction at equilibrium.
The rate of the forward reaction is less than the rate of the reverse reaction at equilibrium.
Discuss the significance of equilibrium constant in determining the extent of a reaction.
The equilibrium constant is a measure of the rate of reaction
The equilibrium constant (Keq) is a measure of the ratio of products to reactants at equilibrium. It indicates how far a reaction has proceeded towards completion. A large Keq value suggests the reaction favors the formation of products, while a small Keq value indicates the reaction favors the formation of reactants. Therefore, the equilibrium constant is crucial in determining the extent to which a reaction occurs.
A large Keq value indicates the reaction favors the formation of reactants
The equilibrium constant is not affected by temperature
What factors can influence the equilibrium position in a heterogeneous system?
Humidity, wind speed, altitude
Number of spectators, type of music playing, brand of shoes worn
Temperature, pressure, concentration of reactants and products, presence of catalysts
Color of the reactants, time of day, phase of the moon
How does the concept of equilibrium relate to the concept of entropy?
Equilibrium and entropy are completely unrelated concepts.
Entropy is a measure of disorder, while equilibrium is a measure of order.
Equilibrium is achieved when entropy is minimized in a system.
Equilibrium and entropy are related as equilibrium represents a state of maximum entropy in a system.
Provide an example of a real-life application of chemical equilibrium principles.
Haber process for ammonia production
Fischer-Tropsch process for synthetic fuel production
Ostwald process for nitric acid production
Contact process for sulfuric acid production
