BackChemical Equilibrium quiz #1
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1/38BackSkip to main contentBackWhat is chemical equilibrium?
Chemical equilibrium is the state in which the concentrations of reactants and products remain constant over time because the forward and reverse reactions occur at the same rate. What is dynamic equilibrium in a chemical reaction?
Dynamic equilibrium is when the forward and reverse reactions continue to occur at equal rates, resulting in constant concentrations of reactants and products. What effect does increasing the concentration of products have on the rate of the reverse reaction in a reversible chemical system?
Increasing the concentration of products would increase the rate of the reverse reaction. What is always true about the rates of forward and reverse reactions at equilibrium?
The rates of the forward and reverse reactions are equal. What happens to the concentrations of reactants and products during a reaction at equilibrium?
The concentrations of reactants and products remain constant over time. When any reversible reaction is at equilibrium, what is true about the rates of the forward and reverse reactions?
The rates of the forward and reverse reactions are equal. What happens to the concentrations of all reactants and products in a system at equilibrium?
The concentrations of all reactants and products remain constant over time. Which set of values tells us if the reaction is at equilibrium?
The concentrations of reactants and products, when plugged into the equilibrium constant expression, match the value of K. Which equation represents a physical equilibrium?
An example is H2O(l) ⇌ H2O(g), representing equilibrium between liquid and vapor phases. Which equation represents a chemical equilibrium?
An example is N2(g) + 3H2(g) ⇌ 2NH3(g), representing equilibrium between reactants and products in a chemical reaction. What is true for a system at chemical equilibrium?
The forward and reverse reactions occur at the same rate. If the concentrations of products and reactants are equal, what does this imply about the equilibrium constant?
The equilibrium constant K is equal to 1. What can be said about the relative amounts of reactants and products when K > 1?
Products are favored and present in greater amounts than reactants. Which statement explains what it means for a chemical reaction to be at equilibrium?
The forward and reverse reactions occur at equal rates, and the concentrations of reactants and products remain constant. Which figure represents the point at which equilibrium is reached in a reaction progress graph?
The point where the concentrations of reactants and products plateau and remain constant. What condition must occur when a chemical reaction is at equilibrium?
The rates of the forward and reverse reactions must be equal. When is a reversible chemical reaction in equilibrium?
When the forward and reverse reaction rates are equal and concentrations remain constant. What happens to the concentrations of reactants and products when a system is at equilibrium?
The concentrations of reactants and products do not change over time. What can be said about the relative amounts of reactants and products when K is approximately 1?
Reactants and products are present in roughly equal amounts. Which phrase defines chemical equilibrium?
A state where the forward and reverse reactions occur at equal rates and concentrations remain constant. What happens to the concentrations of reactants and products once a chemical reaction has reached equilibrium?
The concentrations of reactants and products remain constant, but reactions continue to occur. What happens when a chemical reaction reaches equilibrium?
The forward and reverse reactions occur at the same rate, and concentrations of all species remain constant. Which occurs when the forward and reverse reactions occur at the same rate?
Chemical equilibrium is established. What does it imply when the Keq value is equal to 1?
Reactants and products are present in equal concentrations at equilibrium. What condition must occur when a chemical reaction is at equilibrium?
The rates of the forward and reverse reactions must be equal. What can we conclude when the Keq value is very high?
The reaction strongly favors the formation of products. What are the characteristics of equilibrium?
Constant concentrations of reactants and products, equal rates of forward and reverse reactions, and ongoing molecular activity. Which best describes dynamic equilibrium?
A state where forward and reverse reactions continue at equal rates, keeping concentrations constant. What is the equilibrium constant expression for a general reaction aA + bB ⇌ cC + dD?
K = [C]^c [D]^d / [A]^a [B]^b For a particular reaction K = 98000. What can be said about this reaction?
The reaction strongly favors the formation of products at equilibrium. The equilibria studied in the lab procedure include which two reactants?
The specific reactants depend on the experiment, but typically involve a reversible reaction with identifiable reactants and products. What happens to a reaction system where the reaction quotient Q is less than the equilibrium constant Kc?
The reaction will proceed in the forward direction to reach equilibrium. What is the value of the rate constant for this reaction?
The rate constant value depends on the specific reaction and must be provided or calculated from experimental data. What is a reversible reaction?
A reversible reaction is one in which products can react to reform reactants, allowing the reaction to proceed in both directions. The amount of H2(g) present in a reaction mixture at equilibrium can be maximized by what method?
By shifting the equilibrium toward the side containing H2(g), such as by changing concentrations, pressure, or temperature as appropriate. Choose the option below that is not necessarily true of a system at equilibrium.
The concentrations of reactants and products are equal. What is true about the rates of the forward and reverse reactions in a system at chemical equilibrium?
The forward and reverse reactions occur at equal rates. The value of Kp for the evaporation of CH3OH(l) at 300 K is closest to what?
The value depends on experimental data; it is calculated using the partial pressures of CH3OH(g) and CH3OH(l) at equilibrium.
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