What is the correct equilibrium expression for the following reaction: 2H 2 O 2 (aq) ↔ 2H 2 O(l) + O 2 (g)

[H 2 O] 2 [O 2 ] / [H 2 O 2 ] 2

[H 2 O 2 ] 2 / [H 2 O] 2 [O 2 ]

In which of the following systems would the number of moles of the substances present at equilibrium NOT be shifted by a change in the volume of the system at constant temperature?

NO (g) + O 3 (g) ↔ NO 2 (g) + O 2 (g)

CO (g) + NO (g) ↔ CO 2(g) + ½N 2(g)

Which of the following shows the correct dissolution reaction for BaCl 2 ?

BaCl 2 (s) -> Ba 2+ (aq) + 2Cl - (aq)

Ba 2+ (aq) + Cl 2 - (aq) -> BaCl 2 (s)

BaCl 2 (aq) -> Ba 2+ (aq) + 2Cl - (aq)

Ba 2+ (aq) + 2Cl - (aq) -> BaCl 2 (s)

Which of the following is NOT true at equilibrium?

The concentration of the reactants is equal to the concentration of the products.

The forward and reverse reactions proceed at the same rate.

The concentrations of reactants and products do not change.

The forward and reverse reactions continue to occur.

What is the equilibrium expression for: Fe 3 O 4 (s) + 4H 2 (g) <--> 3Fe(s) + 4H 2 O(g)

([Fe] 3 [H 2 O] 4 ) / ([Fe 3 O 4 ][H 2 ] 4 )

([Fe 3 O 4 ][H 2 ] 4 )/ ([Fe] 3 [H 2 O] 4 )

([Fe][H 2 O]) / ([Fe 3 O 4 ][H 2 ])

There are more products than reactants when the reaction reached equilibrium.

There are more reactant than products when the reaction reached equilibrium.

The amount of reactants is equal to the amount of products.

The reaction quotient for a system is 7.2 × 10 2 . If the equilibrium constant for the system is 36, what will happen as equilibrium is approached?

There will be a net gain in reactant.

There will be a net gain in product

There will be a net gain in both product and reactant

There will be no net gain in either product or reactant.

AP Chemistry Unit 7 - Equilibrium

Authored by Tricia Kreitzer

Chemistry

11th - 12th Grade

NGSS covered

Used 465+ times

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About

This quiz covers chemical equilibrium, a fundamental topic in AP Chemistry that addresses dynamic chemical systems and their quantitative relationships. The questions assess students' understanding of equilibrium constants (Kc and Ksp), Le Chatelier's principle, reaction quotients, acid-base equilibria, and solubility equilibria. Students need to master the mathematical relationships between equilibrium expressions and concentration data, understand how external factors like temperature, pressure, and concentration changes affect equilibrium position, and apply these concepts to real chemical systems. The content requires strong algebraic skills for equilibrium calculations, conceptual understanding of reversible reactions, and the ability to write correct equilibrium expressions while excluding solids and liquids. Students must also understand the relationship between equilibrium constants and reaction favorability, distinguish between strong and weak acids and bases, and solve complex problems involving pH, pOH, and buffer systems. Created by Tricia Kreitzer, a Chemistry teacher in the US who teaches grades 11 and 12. This comprehensive assessment serves as an excellent tool for evaluating student mastery of equilibrium concepts before the AP Chemistry exam. Teachers can use this quiz as a summative assessment after completing Unit 7, as a review activity before the AP exam, or as a diagnostic tool to identify areas where students need additional support. The variety of question types—from conceptual understanding of Le Chatelier's principle to complex equilibrium calculations—makes it suitable for differentiated instruction and allows teachers to assess both conceptual knowledge and mathematical problem-solving skills. This quiz aligns with AP Chemistry Learning Objectives related to equilibrium (LO 6.1-6.21) and supports the College Board's emphasis on connecting macroscopic observations to molecular-level explanations while developing quantitative reasoning skills essential for success in advanced chemistry coursework.

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32 questions

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Given the K_c for a forward reaction, how can you find K_c for the reverse reaction?

Divide K_c by 1

Divide 1 by K_c

Square K_c

Take the square root of K_c

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

For the reaction...
SO₂ + O₂ <−> SO₃
If the concentration of SO₂is increased, the equilibrium of the reaction will shift ___________.

left

right

left and right

neither left nor right

Tags

NGSS.HS-PS1-6

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

For the reaction...
heat + N₂ + O₂ ↔ 2NO
If heat is added to the chemical system, the equilibrium will shift _______.

left

right

left and right

neither left nor right

Tags

NGSS.HS-PS1-6

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

2SO₂(g)+O₂(g)⇌2SO₃(g)
Decreasing the volume of container will

shift equilibrium right

shift equilibrium left

change K

have no change

Tags

NGSS.HS-PS1-6

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

For the reaction...
N₂ + O₂ <=> 2NO
If O₂ is removed, the concentration of N₂ will _______.

increase

decrease

remain the same

double

Tags

NGSS.HS-PS1-6

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

The following reaction :
SO_{2 (g)} + NO_{2 (g)} <=> SO_{3 (g)} + NO (g)
had reached a state of equilibrium, was found to contain
0.40 mol L^-1 SO₃ , and 0.30 mol L^-1 NO,
0.15 mol L^-1NO₂ , and 0.20 mol L^-1 SO₂.
Calculate the equilibrium constant for this reaction.

4.0

0.42

0.25

1.0

Tags

NGSS.HS-PS1-6

MULTIPLE CHOICE QUESTION

45 sec • 1 pt

What are the two factors to look for when determining if the reaction is at equilibrium?

Forward reaction rate is faster than the reverse and concentrations are equal

Forward and reverse reaction rates are equal and concentration is conctant

Forward and revers reaction rates are equal and concentration is equal

Forward reaction rate is faster than the reverse and concentration is equal

Tags

NGSS.HS-PS1-6

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AP Chemistry Unit 7 - Equilibrium

Given the K_c for a forward reaction, how can you find K_c for the reverse reaction?

For the reaction...
SO₂ + O₂ <−> SO₃
If the concentration of SO₂is increased, the equilibrium of the reaction will shift ___________.

For the reaction...
heat + N₂ + O₂ ↔ 2NO
If heat is added to the chemical system, the equilibrium will shift _______.

2SO₂(g)+O₂(g)⇌2SO₃(g)
Decreasing the volume of container will

For the reaction...
N₂ + O₂ <=> 2NO
If O₂ is removed, the concentration of N₂ will _______.

The following reaction :
SO_{2 (g)} + NO_{2 (g)} <=> SO_{3 (g)} + NO (g)
had reached a state of equilibrium, was found to contain
0.40 mol L^-1 SO₃ , and 0.30 mol L^-1 NO,
0.15 mol L^-1NO₂ , and 0.20 mol L^-1 SO₂.
Calculate the equilibrium constant for this reaction.

What are the two factors to look for when determining if the reaction is at equilibrium?

What is [H₂O] if K = 1.2,
[CO₂] = 0.846M, & [CH₄]= 0.0713M?
4CuO_(s)+CH_4(g)↔CO_2(g)+4Cu_(s) +2H₂O_(g)

What is the correct equilibrium expression for the following reaction:
2H₂O₂(aq) ↔ 2H₂O(l) + O₂(g)

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Popular Resources on Wayground

Discover more resources for Chemistry

AP Chemistry Unit 7 - Equilibrium

Given the Kc for a forward reaction, how can you find Kc for the reverse reaction?

For the reaction...SO2 + O2 <−> SO3If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.

For the reaction...heat + N2 + O2 ↔ 2NOIf heat is added to the chemical system, the equilibrium will shift _______.

2SO2(g)+O2(g)⇌2SO3(g)Decreasing the volume of container will

For the reaction...N2 + O2 <=> 2NOIf O2 is removed, the concentration of N2 will _______.

The following reaction : SO2 (g) + NO2 (g) <=> SO3 (g) + NO (g)had reached a state of equilibrium, was found to contain 0.40 mol L-1 SO3 , and 0.30 mol L-1 NO, 0.15 mol L-1NO2 , and 0.20 mol L-1 SO2. Calculate the equilibrium constant for this reaction.

What are the two factors to look for when determining if the reaction is at equilibrium?

What is [H2O] if K = 1.2, [CO2] = 0.846M, & [CH4]= 0.0713M?4CuO(s)+CH4(g)↔CO2(g)+4Cu(s) +2H2O(g)

What is the correct equilibrium expression for the following reaction:2H2O2(aq) ↔ 2H2O(l) + O2(g)

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Given the K_c for a forward reaction, how can you find K_c for the reverse reaction?

For the reaction...
SO₂ + O₂ <−> SO₃
If the concentration of SO₂is increased, the equilibrium of the reaction will shift ___________.

For the reaction...
heat + N₂ + O₂ ↔ 2NO
If heat is added to the chemical system, the equilibrium will shift _______.

2SO₂(g)+O₂(g)⇌2SO₃(g)
Decreasing the volume of container will

For the reaction...
N₂ + O₂ <=> 2NO
If O₂ is removed, the concentration of N₂ will _______.

The following reaction :
SO_{2 (g)} + NO_{2 (g)} <=> SO_{3 (g)} + NO (g)
had reached a state of equilibrium, was found to contain
0.40 mol L^-1 SO₃ , and 0.30 mol L^-1 NO,
0.15 mol L^-1NO₂ , and 0.20 mol L^-1 SO₂.
Calculate the equilibrium constant for this reaction.

What is [H₂O] if K = 1.2,
[CO₂] = 0.846M, & [CH₄]= 0.0713M?
4CuO_(s)+CH_4(g)↔CO_2(g)+4Cu_(s) +2H₂O_(g)

What is the correct equilibrium expression for the following reaction:
2H₂O₂(aq) ↔ 2H₂O(l) + O₂(g)