Why is equilibrium called a dynamic state?

The reactions at equilibrium continue to take place once equilibrium is established.

Chemists try to convert as much reactants as possible into products.

The products of a forward reaction are favored, so equilibrium lies to the right.

All chemical reactions are considered to be reversible under suitable conditions.

What is the K c expression for this reaction? 2 NO (g) + O 2(g) ⇌ 2 NO 2(g)

K c = [NO 2 ] 2 / [NO] 2 [O 2 ]

K c = [NO] 2 [O 2 ] / [NO 2 ] 2

K c = [NO 2 ] 2 / [NO] 2 + [O 2 ]

An equilibrium constant with a large value, e.g. K c = 1000, indicates…

Mostly reactants at equilibrium

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

Forward and reverse reaction rates are equal and concentration is conctant

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

Forward and revers reaction rates are equal and concentration is equal

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

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)

When the chemical reaction A + B ↔ C+ D is at equilibrium,

neither the forward nor the reverse reactions have stopped.

both the forward and reverse reactions have stopped.

the sum of the concentrations of A and B equals the sum of the concentrations of C and D.

all four concentrations are equal.

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.

CuO(s) + H 2 (g) ↔ Cu(s) + H 2 O(g) ΔH = –2.0 kilojoules mol –1 When the substances in the equation above are at equilibrium at pressure P and temperature T , the equilibrium can be shifted to favor the products by

increasing the pressure by means of a moving piston at constant T

increasing the pressure by adding an inert gas such as nitrogen

An equilibrium constant with a large magnitude indicates…

Higher concentration of products at equilibrium

Higher concentration of reactants at equilibrium

Nothing, without considering the stoichiometry of the reaction

H 2 ( g ) + I 2 ( g ) ⇄ 2 HI( g ) At 450 o C, 2.0 moles each of H 2 ( g ), I 2 ( g ), and HI( g ) are combined in a 1.0 L rigid container. The value of K c at 450 o C is 50. Which of the following will occur as the system moves toward equilibrium?

More H 2 ( g ) and I 2 ( g ) will form.

The total pressure will decrease.

No net reaction will occur, because the number of molecules is the same on both sides of the equation.

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.

AP Chemistry Equilibrium and Ksp

Authored by M Garcia

Chemistry

10th - 12th Grade

NGSS covered

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MULTIPLE CHOICE QUESTION

5 mins • 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

5 mins • 1 pt

This endothermic reaction is at equilibrium.
If its temperature is increased (at constant volume and pressure), which way will the equilibrium shift?

To products (right)

To reactants (left)

Tags

NGSS.HS-PS1-6

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

Le Chatelier's Principle states that if a chemical system at equilibrium is stressed,

the system will adjust to increase the stress

the system will adjust to reduce the stress

the system will not adjust

Tags

NGSS.HS-PS1-6

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

This symbol indicates that a reaction is ____________

reversible

irreversible

Tags

NGSS.HS-PS1-6

MULTIPLE CHOICE QUESTION

5 mins • 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

5 mins • 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

5 mins • 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

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AP Chemistry Equilibrium and Ksp

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

This endothermic reaction is at equilibrium.
If its temperature is increased (at constant volume and pressure), which way will the equilibrium shift?

Le Chatelier's Principle states that if a chemical system at equilibrium is stressed,

This symbol indicates that a reaction is ____________

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

At what time (in seconds) is equilibrium established?

Why is equilibrium called a dynamic state?

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

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Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

AP Chemistry Equilibrium and Ksp

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

This endothermic reaction is at equilibrium.If its temperature is increased (at constant volume and pressure), which way will the equilibrium shift?

Le Chatelier's Principle states that if a chemical system at equilibrium is stressed,

This symbol indicates that a reaction is ____________

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

At what time (in seconds) is equilibrium established?

Why is equilibrium called a dynamic state?

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

Access all questions and much more by creating a free account

Similar Resources on Wayground

Popular Resources on Wayground

Discover more resources for Chemistry

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

This endothermic reaction is at equilibrium.
If its temperature is increased (at constant volume and pressure), which way will the equilibrium shift?

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 _______.