In an experiment, Louis and Umar added radioactive Pb*(NO 3 ) 2 (aq) to the following equilibrium system: [* indicates radioactive Pb 2+ ions] PbCl 2 (s) ↔ Pb 2+ (aq) + 2Cl − (aq). When equilibrium was re-established, some of the PbCl 2 (s) was recovered from the system and dried. Testing showed the PbCl 2 (s) was radioactive. Which statement is best supported by this result?

The process of dynamic equilibrium is demonstrated.

At equilibrium, the rates of chemical change are equal.

At equilibrium, the rates of chemical change are unequal.

The process of dynamic equilibrium is not demonstrated.

Louis and Jaeda are calibrating a Celsius thermometer at 1 atmosphere of pressure. The fixed temperature points they use are determined on the basis of

both the ice/water and the water/steam equilibrium temperatures

the ice/water equilibrium temperature only

the water/steam equilibrium temperature only

neither the ice/water nor the water/steam equilibrium temperatures

Jaeda and Deshaun are conducting an experiment with copper(II) sulfate. They observe the reaction: CuSO 4 (s) ↔ $$Cu^{2+}(aq)$$ + $$SO_4^{2-}(aq)$$ . When they powder the CuSO 4 (s), it dissolves more rapidly. This is because the increased surface area due to powdering permits:

the equilibrium to shift to the left

the equilibrium to shift to the right

Christopher and Louis are conducting an experiment where a chemical reaction is at equilibrium. What will happen if they add a catalyst to the system?

The rates of the forward and reverse reactions will change.

The equilibrium concentration of AB will increase.

The equilibrium concentration of AB will decrease.

The equilibrium constant for the reaction will change.

Umar and Deshaun are conducting an experiment with the reaction at equilibrium: 2 SO 2 (g) + O 2 (g) ↔ 2 SO 3 (g). If the temperature remains constant, an increase in pressure will:

shift the equilibrium to the right

have no effect on the equilibrium

shift the equilibrium to the left

change the value of the equilibrium constant

Damilola and Umar are using a chemical cell in their science experiment. What does it indicate when the voltage (E⁰) of their chemical cell drops to zero?

The cell reaction has reached equilibrium.

The concentration of the reactants has increased.

The concentration of the products has decreased.

The cell reaction has completely stopped.

Danny and Jaeda are conducting an experiment in a closed system with the following equilibrium reaction: H 2 (g) + I 2 (g) + heat ↔ 2 HI(g). What will be the result of an increase in temperature?

The equilibrium will shift to the right and [HI] will increase.

The equilibrium will shift to the left and [H 2 ] will increase.

The equilibrium will shift to the left and [HI] will decrease.

The equilibrium will shift to the right and [HI] will decrease.

Christopher and Jaeda are conducting an experiment with carbonated water. According to Le Chatelier's principle, if they decrease the concentration of CO 2 in the water, what will happen?

Decrease the concentration of H 2 CO 3

Increase the concentration of H 2 CO 3

Have no effect on the concentration of H 2 CO 3

Increase the concentration of CO 2

Deshaun and Jaeda are conducting an experiment to dissolve KNO 3 in water. According to Le Chatelier's principle, why does an increase in temperature increase the solubility of KNO 3 ?

Because the dissolution of KNO 3 is endothermic, and increasing temperature shifts the equilibrium to favor more dissolution.

Because the dissolution of KNO 3 is exothermic, and increasing temperature shifts the equilibrium to favor less dissolution.

Because increasing temperature decreases the kinetic energy of the molecules.

Because KNO 3 decomposes at higher temperatures.

Umar and Jordan are dissolving KNO 3 in water for a science experiment. They notice that after a certain point, no more KNO 3 seems to dissolve, and some remains at the bottom. In terms of equilibrium, a solution is saturated when:

the rate of dissolution equals the rate of precipitation

all of the solute has dissolved

Danny and Jordan are studying a potential energy diagram for a chemical reaction in their science class. Which of the following must be shown on the potential energy diagram for the forward reaction?

Activation energy and potential energy of the products

Only the potential energy of the products

Neither activation energy nor potential energy of the products

Christopher and Jaeda are observing a chemical reaction in their science class. They notice that the reaction vessel feels warm to the touch. Explain, in terms of energy, why the reaction is classified as exothermic.

Because energy is released to the surroundings.

Because energy is absorbed from the surroundings.

Because no energy change occurs.

Because energy is converted to mass.

Damilola and Deshaun are studying the synthesis of ammonia, NH 3 (g), in their chemistry class. According to Le Chatelier's principle, the concentration of NH 3 (g) decreases when the temperature of the equilibrium system increases because:

The forward reaction is exothermic and increasing temperature favors the reverse reaction.

The forward reaction is endothermic and increasing temperature favors the forward reaction.

The system produces more NH 3 to counteract the temperature increase.

Temperature has no effect on the equilibrium position.

Danny and Louis add solid KCl to water in a flask. The flask is sealed with a stopper and thoroughly shaken until no more solid KCl dissolves. Some solid KCl is still visible in the flask. The solution in the flask is

saturated and is at equilibrium with the solid KCl

saturated and is not at equilibrium with the solid KCl

unsaturated and is at equilibrium with the solid KCl

unsaturated and is not at equilibrium with the solid KCl

Jaeda and Christopher are conducting an experiment involving a reaction that produces SO 2 (g). According to Le Chatelier's principle, the concentration of SO 2 (g) increases when the temperature is increased because:

The forward reaction is exothermic.

The reaction is unaffected by temperature.

SO 2 is removed from the system.

During a science experiment, Umar and Jaeda are observing the reaction: 2 SO 2 (g) + O 2 (g) ⇌ 2 SO 3 (g) + energy. When they increase the concentration of O 2 (g), they notice a decrease in the concentration of SO 2 (g). This happens because:

It increases the number of collisions between O 2 and SO 2 molecules, leading to more SO 3 being formed.

It decreases the energy of the system, favoring the reverse reaction.

It reduces the number of SO 2 molecules available for reaction.

It causes SO 2 to decompose spontaneously.

27. Christopher and Jaeda are observing a chemical reaction at equilibrium: 2NO 2 (g) ⇌ N 2 O 4 (g) + 55.3 kJ. The reaction is exothermic in the forward direction because:

Energy is released when N 2 O 4 is formed.

Energy is absorbed when N 2 O 4 is formed.

Energy is absorbed when NO 2 is formed.

28. Umar and Jaeda are conducting an experiment with a sealed container in which the following reaction is at equilibrium: 2NO 2 (g) ⇌ N 2 O 4 (g) + 55.3 kJ According to Le Chatelier's principle, when they increase the pressure on the system at constant temperature, the equilibrium shifts to the right because:

The forward reaction produces fewer moles of gas.

The forward reaction produces more moles of gas.

The reverse reaction produces fewer moles of gas.

The reverse reaction produces more moles of gas.

Jordan and Damilola are conducting an experiment with the system at equilibrium: 2POCl 3 (g) + energy ⇌ 2PCl 3 (g) + O 2 (g). Which changes occur when O 2 (g) is added to this system?

The equilibrium shifts to the left and the concentration of PCl 3 (g) decreases.

The equilibrium shifts to the right and the concentration of PCl 3 (g) increases.

The equilibrium shifts to the right and the concentration of PCl 3 (g) decreases.

The equilibrium shifts to the left and the concentration of PCl 3 (g) increases.

30. Jordan and Umar are learning about the manufacture of a bleaching solution in their chemistry class. The equilibrium equation below is related to this process. In this equation, Cl - (aq) means that chloride ions are surrounded by water molecules. Cl 2 (g) + 2 OH - (aq) ⇌ OCl - (aq) + Cl - (aq) Use the key to draw two water molecules in the box, showing the correct orientation of each water molecule toward the chloride ion.

The two water molecules should be drawn with their hydrogen atoms pointing toward the Cl - ion, as the positive hydrogen ends are attracted to the negative chloride ion.

The two water molecules should be drawn with their oxygen atoms pointing toward the Cl - ion, as the negative oxygen ends are attracted to the negative chloride ion.

The two water molecules should be drawn with their hydrogen atoms pointing away from the Cl - ion, as the positive hydrogen ends repel the negative chloride ion.

The two water molecules should be drawn with their oxygen atoms pointing away from the Cl - ion, as the negative oxygen ends repel the negative chloride ion.

Jaeda and Damilola are conducting an experiment with chlorine gas. They observe that increasing the concentration of Cl 2 (g) increases the concentration of OCl - (aq) in their equilibrium system because, according to collision theory:

It increases the frequency of effective collisions between reactant particles, leading to a higher rate of the forward reaction.

It decreases the activation energy required for the reaction to occur.

It increases the temperature of the system, favoring the formation of OCl - (aq).

It changes the equilibrium constant of the reaction.

32. Deshaun and Umar are conducting an experiment with a beaker containing 100.0 milliliters of a dilute aqueous solution of ethanoic acid at equilibrium. The equation below represents this system: HC 2 H 3 O 2 (aq) ⇌ H + (aq) + C 2 H 3 O 2 - (aq). At equilibrium, the rate of the forward reaction is:

equal to the rate of the reverse reaction

greater than the rate of the reverse reaction

less than the rate of the reverse reaction

During a chemistry experiment, Danny and Jaeda add 10 drops of concentrated HC 2 H 3 O 2 (aq) to a solution. Describe what happens to the concentration of H + (aq) in the system.

The concentration of H + (aq) increases.

The concentration of H + (aq) decreases.

The concentration of H + (aq) remains the same.

The concentration of H + (aq) first increases, then decreases.

Jordan and Damilola are observing a chemical reaction in the lab. They record the concentrations of reactants and products over time, as shown in the graph. What information on the graph indicates that the system was initially at equilibrium?

The concentrations of reactants and products remain constant at the beginning.

The temperature of the system increases at the start.

The pressure of the system decreases initially.

The graph shows a sudden spike in concentration at the start.

During a chemistry experiment, Deshaun and Damilola observed the reaction between nitrogen, hydrogen, and ammonia gases. According to Le Chatelier's principle, the final concentration of NH₃(g) is greater than the initial concentration of NH₃(g) because:

the system shifts to produce more NH₃(g) when a change is applied

the system shifts to consume NH₃(g) when a change is applied

NH₃(g) decomposes spontaneously

Umar and Louis are conducting an experiment with hydrogen gas, H₂(g), in a closed system. They add more H₂(g) to the system and observe the changes. Explain, in terms of collision theory, why the concentration of H₂(g) begins to decrease immediately after Umar and Louis add more H₂(g) to the system.

Because the rate of collisions between H₂(g) molecules and other reactant molecules increases, leading to a faster reaction.

Because the temperature of the system decreases, causing H₂(g) to react more quickly.

Because the pressure decreases, causing H₂(g) to escape from the system.

Because the concentration of other reactants decreases, slowing down the reaction.

Christopher and Jaeda are working on a chemistry experiment involving the reaction: N 2 (g) + 3H 2 (g) ↔ 2NH 3 (g). What occurs when they increase the concentration of H 2 (g) in their experiment?

The equilibrium shifts to the right, and the concentration of N 2 (g) decreases.

The equilibrium shifts to the left, and the concentration of N 2 (g) decreases.

The equilibrium shifts to the left, and the concentration of N 2 (g) increases.

The equilibrium shifts to the right, and the concentration of N 2 (g) increases.

Louis and Damilola are conducting an experiment with gases in a cylinder. They notice that increasing the pressure of the gases in the cylinder increases the rate of the forward reaction because, according to collision theory:

It increases the concentration of gas molecules, leading to more frequent collisions.

It increases the temperature of the gases.

It decreases the activation energy required for the reaction.

It changes the products formed in the reaction.

Deshaun and Louis are conducting an experiment with the reaction at equilibrium involving SO 3 (g). State, in terms of the concentration of SO 3 (g), what happens when more O 2 (g) is added to the reaction at equilibrium.

The concentration of SO 3 (g) increases.

The concentration of SO 3 (g) decreases.

The concentration of SO 3 (g) remains the same.

The concentration of SO 3 (g) becomes zero.

Deshaun and Damilola are investigating a chemical reaction in their science class. On the labeled axes below, which option correctly completes the potential energy diagram for the forward reaction they are studying, as represented by this equation?

A diagram showing a decrease in potential energy from reactants to products, with an activation energy peak.

A diagram showing a constant potential energy from reactants to products.

A diagram showing an increase in potential energy from reactants to products, with no activation energy peak.

A diagram showing random fluctuations in potential energy.

Umar and Danny are observing a chemical reaction in their science class. Compare the rate of the forward reaction with the rate of the reverse reaction for this system.

The forward rate is greater than the reverse rate.

The reverse rate is greater than the forward rate.

During a chemistry experiment, Damilola and Louis are observing a reaction in a container. The container must be closed to maintain equilibrium because:

It prevents the escape of reactants or products, allowing equilibrium to be established.

It allows more heat to enter the system.

It increases the pressure inside the container.

It speeds up the reaction rate.

At equilibrium, the rates of the forward and reverse reactions are:

Greater for the forward reaction

Greater for the reverse reaction

The equation below represents an equilibrium system of SO₂(g), O₂(g), and SO₃(g). The reaction can be catalyzed by vanadium or platinum. 2SO₂(g) + O₂(g) ⇌ 2SO₃(g) + energy A potential energy diagram for the forward reaction is shown above. On this diagram, which of the following best represents how the potential energy changes when the reaction occurs by the catalyzed pathway?

A dashed line showing a lower activation energy than the uncatalyzed pathway

A dashed line showing a higher activation energy than the uncatalyzed pathway

A dashed line at the same activation energy as the uncatalyzed pathway

A dashed line showing no change in potential energy

Chemical Equilibrium and Thermodynamics Worksheet

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79 Qs

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Chemical Equilibrium and Thermodynamics Worksheet

Quiz

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Chemistry

•

11th Grade

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Practice Problem

•

Hard

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NGSS

HS-PS1-5, HS-PS1-6, HS-PS1-4

Standards-aligned

Mr. Poyser

Used 1+ times

FREE Resource

79 questions

Show all answers

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Umar and Louis are observing a chemical reaction in their science class. Which statement is true if the free energy (ΔG) of the reaction they are studying is zero?

The rate of the forward reaction is zero.

The rate of the reverse reaction is zero.

The reaction is approaching equilibrium.

The reaction is at equilibrium.

Answer explanation

When the free energy (ΔG) of a reaction is zero, it indicates that the forward and reverse reactions occur at the same rate, meaning the system is at equilibrium.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

During a chemistry experiment, Danny and Damilola add a catalyst to a reaction mixture that has reached equilibrium. The value of the equilibrium constant

decreases

increases

remains the same

Answer explanation

A catalyst speeds up the rate of reaching equilibrium but does not change the position of equilibrium or the value of the equilibrium constant. Therefore, the equilibrium constant remains the same.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Jaeda and Umar are conducting an experiment. If they increase the temperature of a chemical system at constant pressure, the rate of the forward reaction will

decrease

increase

remain the same

Answer explanation

Increasing the temperature at constant pressure typically favors the endothermic direction of a reaction. If the forward reaction is endothermic, its rate will increase with temperature, making 'increase' the correct choice.

During a chemistry experiment, Deshaun and Jaeda are observing a reaction in a closed container. If O₂ is added to the system at constant pressure and temperature, what will happen to the number of moles of HCl?

decrease

increase

remain the same

Answer explanation

Adding O2 shifts the equilibrium of the reaction involving HCl, leading to a decrease in the concentration of HCl as it reacts to form products. Therefore, the number of moles of HCl will decrease.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Jaeda and Damilola are conducting an experiment with a chemical reaction at constant temperature. If they increase the pressure on the system, the value of the equilibrium constant for the reaction will

decrease

increase

remain the same

Answer explanation

Increasing pressure shifts the equilibrium towards the side with fewer moles of gas. If the reaction produces more moles of gas, the equilibrium constant will increase, making the correct answer 'increase'.

During a science experiment, Umar and Jaeda are investigating phase changes at 1 atmosphere of pressure. Which equilibrium is correctly associated with the Kelvin temperature at which it occurs?

ice-water equilibrium at 0 K

ice-water equilibrium at 32 K

steam-water equilibrium at 212 K

steam-water equilibrium at 373 K

Answer explanation

The steam-water equilibrium occurs at 373 K (100°C) at 1 atmosphere pressure, which is the boiling point of water. The other options incorrectly associate temperatures with their respective equilibria.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Jaeda and Danny place a sealed flask of water at 298 K on their classroom desk. After some time, the water is in equilibrium with its vapor inside the flask. This is an example of:

chemical equilibrium

phase equilibrium

solution equilibrium

static equilibrium

Answer explanation

This scenario illustrates phase equilibrium, where liquid water and its vapor coexist in a sealed environment at a constant temperature. The system is balanced between the liquid and vapor phases.

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Chemical Equilibrium and Thermodynamics Worksheet

79 questions

Umar and Louis are observing a chemical reaction in their science class. Which statement is true if the free energy (ΔG) of the reaction they are studying is zero?

When the free energy (ΔG) of a reaction is zero, it indicates that the forward and reverse reactions occur at the same rate, meaning the system is at equilibrium.

During a chemistry experiment, Danny and Damilola add a catalyst to a reaction mixture that has reached equilibrium. The value of the equilibrium constant

A catalyst speeds up the rate of reaching equilibrium but does not change the position of equilibrium or the value of the equilibrium constant. Therefore, the equilibrium constant remains the same.

Jaeda and Umar are conducting an experiment. If they increase the temperature of a chemical system at constant pressure, the rate of the forward reaction will

Increasing the temperature at constant pressure typically favors the endothermic direction of a reaction. If the forward reaction is endothermic, its rate will increase with temperature, making 'increase' the correct choice.

During a chemistry experiment, Deshaun and Jaeda are observing a reaction in a closed container. If O₂ is added to the system at constant pressure and temperature, what will happen to the number of moles of HCl?

Adding O2 shifts the equilibrium of the reaction involving HCl, leading to a decrease in the concentration of HCl as it reacts to form products. Therefore, the number of moles of HCl will decrease.

Jaeda and Damilola are conducting an experiment with a chemical reaction at constant temperature. If they increase the pressure on the system, the value of the equilibrium constant for the reaction will

Increasing pressure shifts the equilibrium towards the side with fewer moles of gas. If the reaction produces more moles of gas, the equilibrium constant will increase, making the correct answer 'increase'.

During a science experiment, Umar and Jaeda are investigating phase changes at 1 atmosphere of pressure. Which equilibrium is correctly associated with the Kelvin temperature at which it occurs?

The steam-water equilibrium occurs at 373 K (100°C) at 1 atmosphere pressure, which is the boiling point of water. The other options incorrectly associate temperatures with their respective equilibria.

Jaeda and Danny place a sealed flask of water at 298 K on their classroom desk. After some time, the water is in equilibrium with its vapor inside the flask. This is an example of:

This scenario illustrates phase equilibrium, where liquid water and its vapor coexist in a sealed environment at a constant temperature. The system is balanced between the liquid and vapor phases.

The presence of radioactive Pb in the recovered PbCl2(s) indicates that Pb2+ ions were in equilibrium with the solid. This supports the idea of dynamic equilibrium, where both forward and reverse reactions occur at equal rates.

Louis and Jaeda are calibrating a Celsius thermometer at 1 atmosphere of pressure. The fixed temperature points they use are determined on the basis of

The Celsius thermometer is based on two fixed points: the ice/water equilibrium temperature (0°C) and the water/steam equilibrium temperature (100°C) at 1 atmosphere of pressure, making the correct choice both these temperatures.

Powdering CuSO4 increases its surface area, allowing more solvent to contact the solute. This enhances the dissolution rate, making the reaction proceed more towards the right, but the key reason is the increased solvent contact.

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Chemical Equilibrium and Thermodynamics Worksheet

79 questions

Umar and Louis are observing a chemical reaction in their science class. Which statement is true if the free energy (ΔG) of the reaction they are studying is zero?

When the free energy (ΔG) of a reaction is zero, it indicates that the forward and reverse reactions occur at the same rate, meaning the system is at equilibrium.

During a chemistry experiment, Danny and Damilola add a catalyst to a reaction mixture that has reached equilibrium. The value of the equilibrium constant

A catalyst speeds up the rate of reaching equilibrium but does not change the position of equilibrium or the value of the equilibrium constant. Therefore, the equilibrium constant remains the same.

Jaeda and Umar are conducting an experiment. If they increase the temperature of a chemical system at constant pressure, the rate of the forward reaction will

Increasing the temperature at constant pressure typically favors the endothermic direction of a reaction. If the forward reaction is endothermic, its rate will increase with temperature, making 'increase' the correct choice.

During a chemistry experiment, Deshaun and Jaeda are observing a reaction in a closed container. If O2 is added to the system at constant pressure and temperature, what will happen to the number of moles of HCl?

Adding O2 shifts the equilibrium of the reaction involving HCl, leading to a decrease in the concentration of HCl as it reacts to form products. Therefore, the number of moles of HCl will decrease.

Jaeda and Damilola are conducting an experiment with a chemical reaction at constant temperature. If they increase the pressure on the system, the value of the equilibrium constant for the reaction will

Increasing pressure shifts the equilibrium towards the side with fewer moles of gas. If the reaction produces more moles of gas, the equilibrium constant will increase, making the correct answer 'increase'.

During a science experiment, Umar and Jaeda are investigating phase changes at 1 atmosphere of pressure. Which equilibrium is correctly associated with the Kelvin temperature at which it occurs?

The steam-water equilibrium occurs at 373 K (100°C) at 1 atmosphere pressure, which is the boiling point of water. The other options incorrectly associate temperatures with their respective equilibria.

Jaeda and Danny place a sealed flask of water at 298 K on their classroom desk. After some time, the water is in equilibrium with its vapor inside the flask. This is an example of:

This scenario illustrates phase equilibrium, where liquid water and its vapor coexist in a sealed environment at a constant temperature. The system is balanced between the liquid and vapor phases.

The presence of radioactive Pb in the recovered PbCl2(s) indicates that Pb2+ ions were in equilibrium with the solid. This supports the idea of dynamic equilibrium, where both forward and reverse reactions occur at equal rates.

Louis and Jaeda are calibrating a Celsius thermometer at 1 atmosphere of pressure. The fixed temperature points they use are determined on the basis of

The Celsius thermometer is based on two fixed points: the ice/water equilibrium temperature (0°C) and the water/steam equilibrium temperature (100°C) at 1 atmosphere of pressure, making the correct choice both these temperatures.

Powdering CuSO4 increases its surface area, allowing more solvent to contact the solute. This enhances the dissolution rate, making the reaction proceed more towards the right, but the key reason is the increased solvent contact.

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During a chemistry experiment, Deshaun and Jaeda are observing a reaction in a closed container. If O₂ is added to the system at constant pressure and temperature, what will happen to the number of moles of HCl?