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.

Which one of the following will change the value of an equilibrium constant?

adding other substances that do not react with any of the species involved in the equilibrium

varying the initial concentrations of reactants

varying the initial concentrations of products

changing the volume of the reaction vessel

2 BaO 2 ( s ) ⇄ 2 BaO( s ) + O 2 ( g ) Δ H °= 162 kJ/mol rxn APMCQ: A sealed rigid vessel contains BaO 2 ( s ) in equilibrium with BaO( s ) and O 2 ( g ) as represented by the equation above. Which of the following changes will increase the amount of BaO 2 ( s ) in the vessel?

Removing a small amount of O 2 ( g )

Removing a small amount of BaO( s )

2 XY( g ) ⇄ X 2 ( g ) + Y 2 ( g ) K p = 230 A certain gas, XY( g ), decomposes as represented by the equation above. A sample of each of the three gases is put in a previously evacuated container. The initial partial pressures of the gases are shown in the table above. APMCQ: The temperature of the reaction mixture is held constant. In which direction will the reaction proceed?

The reaction will form more reactant.

The reaction will form more products.

The mixture is at equilibrium, so there will be no change.

It cannot be determined unless the volume of the container is known.

CaCO 3 ( s ) ⇄ CaO( s ) + CO 2 (g) ΔH° = 178 kJ/mol rxn APMCQ: The reaction system represented above is at equilibrium. Which of the following will decrease the amount of CaO( s ) in the system?

Lowering the temperature of the system

Increasing the volume of the reaction vessel at constant temperature

Removing some CO 2 ( g ) at constant temperature

Removing some CaCO 3 ( s ) at constant temperature

CdF 2 (s)⇄Cd 2+ (aq)+2F − (aq) APMCQ: A saturated aqueous solution of CdF 2 is prepared. The equilibrium in the solution is represented above. In the solution, [Cd 2+ ] eq =0.0585 M and [F − ] eq =0.117 M. Some 0.90M NaF is added to the saturated solution. Which of the following identifies the molar solubility of CdF 2 in pure water and explains the effect that the addition of NaF has on this solubility?

The molar solubility of CdF 2 in pure water is 0.0585 M, and adding NaF decreases this solubility because the equilibrium shifts to favor the precipitation of some CdF 2 .

The molar solubility of CdF 2 in pure water is 0.0585 M, and adding NaF has no effect on the solubility because only changes in temperature can increase or decrease the molar solubility of an ionic solid.

The molar solubility of CdF 2 in pure water is 0.117M, and adding NaF decreases this solubility because the equilibrium shifts to favor the precipitation of some CdF 2 .

The molar solubility of CdF 2 in pure water is 0.176 M, and adding NaF increases this solubility because the Na + ions displace the Cd 2+ ions, causing the equilibrium to shift to favor the products.

APMCQ: For which of the equilibrium systems represented below will the amount of product(s) at equilibrium increase if the volume of the reaction vessel is increased at a constant temperature?

PCl 5 ( g ) ⇄ PCl 3 ( g ) + Cl 2 ( g )

N 2 ( g ) + O 2 ( g ) ⇄ 2 NO( g )

2 CO( g ) ⇄ C( s ) + CO 2 ( g )

2 BaO2(s) ⇄ 2 BaO(s) + O2(g) ΔH°= 162 kJ/molrxn A sealed rigid vessel contains BaO2(s) in equilibrium with BaO(s) and O2(g) as represented by the equation above. Which of the following changes will increase the amount of BaO2(s) in the vessel?

Removing a small amount of O2( g )

Removing a small amount of BaO( s )

2 H2O(l) ⇄ H3O+(aq) + OH-(aq) The autoionization of water is represented by the equation above. Values of pKw at various temperatures are listed in the table above: Based on the information above, which of the following statements is true?

As the temperature increases, the pH of pure water decreases.

The dissociation of water is an exothermic process.

The pH of pure water is 7.00 at any temperature.

As the temperature increases, the pH of pure water increases.

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.

Equilibrium for 2CrO 4 2- + 2H + →Cr 2 O 7 2- + H 2 O. What happen when OH - ions are added to the system?

Color of system will turn from orange to yellow

Position of equilibrium will shift to right

OH - ions will not react, and thus no change is seen.

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

the system will adjust to reduce the stress

the system will adjust to increase the stress

AP Chemistry Thermodynamics

Authored by Charles Martinez

Chemistry

11th Grade - University

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MULTIPLE CHOICE QUESTION

1 min • 1 pt

For the reaction...
SO₂ + O₂ <−> SO₃If the equilibrium shifts to the right, the concentration of O₂ will ___________.

increase

decrease

remain the same

double

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

MULTIPLE CHOICE QUESTION

1 min • 1 pt

For the reaction...
SO₂ + O₂ <−> SO₃
If the concentration of O₂is decreased, the equilibrium of the reaction will shift ___________.

left

right

left and right

neither left nor right

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Which of the following is NOT true at equilibrium?

The forward and reverse reactions proceed at the same rate.

The concentrations of reactants and products do not change.

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

The forward and reverse reactions continue to occur.

Tags

NGSS.HS-PS1-6

MULTIPLE CHOICE QUESTION

1 min • 1 pt

What is the equilibrium expression for:
Fe₃O₄(s) + 4H₂(g) <--> 3Fe(s) + 4H₂O(g)

([Fe]³[H₂O]⁴ ) / ([Fe₃O₄][H₂]⁴)

([Fe₃O₄][H₂]⁴)/ ([Fe]³[H₂O]⁴)

[H₂O]⁴ / [H₂]⁴

([Fe][H₂O]) / ([Fe₃O₄][H₂])

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Consider the following equation: CO_(g) + 2H_2(g)⇌ CH₃OH_(g)+ Heat
Which of the factors below would decrease the concentration of CH₃OH at equilibrium?

adding CO

incresing H₂

decrease in the temperature

increasing the temperature

Tags

NGSS.HS-PS1-5

MULTIPLE CHOICE QUESTION

1 min • 1 pt

Predict the effect of decreasing the volume of the container on the following reaction:
2NH₃(g) ⇋ N₂(g) + 3H₂(g)

shift left

shift right

no change

all the above

MULTIPLE CHOICE QUESTION

1 min • 1 pt

What is the proper K_eq for the following reaction?
2 NO_(g) + O_2(g) ⇌2 NO_2(g)

K_eq= [NO₂]² / [NO]²[O₂]

K_eq= [NO]²[O₂] / [NO₂]²

K_eq= [NO]²[O₂][NO₂]²

K_eq= 2[NO][O₂] / 2[NO₂]

Tags

NGSS.HS-PS1-6

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AP Chemistry Thermodynamics

For the reaction...
SO₂ + O₂ <−> SO₃If the equilibrium shifts to the right, the concentration of O₂ will ___________.

For the reaction...
SO₂ + O₂ <−> SO₃
If the concentration of O₂is decreased, the equilibrium of the reaction will shift ___________.

Which of the following is NOT true at equilibrium?

What is the equilibrium expression for:
Fe₃O₄(s) + 4H₂(g) <--> 3Fe(s) + 4H₂O(g)

Consider the following equation: CO_(g) + 2H_2(g)⇌ CH₃OH_(g)+ Heat
Which of the factors below would decrease the concentration of CH₃OH at equilibrium?

Predict the effect of decreasing the volume of the container on the following reaction:
2NH₃(g) ⇋ N₂(g) + 3H₂(g)

What is the proper K_eq for the following reaction?
2 NO_(g) + O_2(g) ⇌2 NO_2(g)

What are [A] and [B]?

For reaction a<-- --> b. Use the graph to determine what the Keq will be.

(Calculator Allowed) 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)

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AP Chemistry Thermodynamics

For the reaction...SO2 + O2 <−> SO3If the equilibrium shifts to the right, the concentration of O2 will ___________.

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

Which of the following is NOT true at equilibrium?

What is the equilibrium expression for: Fe3O4(s) + 4H2(g) <--> 3Fe(s) + 4H2O(g)

Consider the following equation: CO(g) + 2H2(g) ⇌ CH3OH(g) + Heat Which of the factors below would decrease the concentration of CH3OH at equilibrium?

Predict the effect of decreasing the volume of the container on the following reaction: 2NH3(g) ⇋ N2(g) + 3H2(g)

What is the proper Keq for the following reaction? 2 NO(g) + O2(g) ⇌2 NO2(g)

What are [A] and [B]?

For reaction a<-- --> b. Use the graph to determine what the Keq will be.

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

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For the reaction...
SO₂ + O₂ <−> SO₃If the equilibrium shifts to the right, the concentration of O₂ will ___________.

For the reaction...
SO₂ + O₂ <−> SO₃
If the concentration of O₂is decreased, the equilibrium of the reaction will shift ___________.

What is the equilibrium expression for:
Fe₃O₄(s) + 4H₂(g) <--> 3Fe(s) + 4H₂O(g)

Consider the following equation: CO_(g) + 2H_2(g)⇌ CH₃OH_(g)+ Heat
Which of the factors below would decrease the concentration of CH₃OH at equilibrium?

Predict the effect of decreasing the volume of the container on the following reaction:
2NH₃(g) ⇋ N₂(g) + 3H₂(g)

What is the proper K_eq for the following reaction?
2 NO_(g) + O_2(g) ⇌2 NO_2(g)

(Calculator Allowed) 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)