A saturated solution of NaBr has a concentration of 45% NaBr in water. What is its solubility in water?

A saturated solution of NaBr has a concentration of 45% NaBr in water. What is its solubility in water?

A)
82 g / 100 g H2O
B)
4.5 g / 100 g H2O
C)
55 g / 100 g H2O
D)
45 g / 100 g H2O

Answer: Not Available

Which of the following Solubility Product expressions below belongs to the following equilibrium reaction. Fe(OH)3(s) ←→Fe3+(aq) + 3OH-(aq)

Which of the following Solubility Product expressions below belongs to the following equilibrium reaction.
Fe(OH)3(s) ←→Fe3+(aq) + 3OH-(aq)

A) Ksp = [Fe3+] x 3 x [OH-]

B) Ksp =[Fe3+] x [OH−]3[Fe(OH)3]
C) Ksp = [Fe3+] x [OH-]

D) Ksp = [Fe3+] x [OH-]3


Answer D

A reaction is considered to be at equilibrium when the rate of the forward reaction is equal to rate of the reverse reaction.

A reaction is considered to be at equilibrium when the rate of the forward reaction is equal to rate of the reverse reaction.

Answer: TRUE

CaCO3 is considered insoluble in water. CaCO3(s) ↔ Ca2+(aq) + CO32-(aq) Which of the following is true about its equilibrium constant?

CaCO3 is considered insoluble in water.
CaCO3(s) ↔ Ca2+(aq) + CO32-(aq)
Which of the following is true about its equilibrium constant?

A) Kc = 1

B) Kc << 1

C) Kc >> 1

Answer B

What is the ionic equation for the dissolution of magnesium phosphate, Mg3(PO4)2?

What is the ionic equation for the dissolution of magnesium phosphate, Mg3(PO4)2?

A) Mg3(PO4)2(s) ←→Mg32+(aq) + (PO4)22-(aq)

B) Mg3(PO4)2(s) ←→Mg2+(aq) + PO43-(aq)

C) Mg3(PO4)2(s) ←→Mg3(PO4)2(aq)

D) Mg3(PO4)2(s) ←→3Mg2+(aq) + 2PO42-(aq)


Answer D

Consider the following reaction at equilibrium in a closed system: 2NO(g) + Cl2(g) ←→2NOCl(g) + heat What effect will introducing more Cl2(g) to the reaction vessel have on the equilibrium?

Consider the following reaction at equilibrium in a closed system:
2NO(g) + Cl2(g) ←→2NOCl(g) + heat
What effect will introducing more Cl2(g) to the reaction vessel have on the equilibrium?

A) The pressure of NO(g) will go down.

B) The pressure of NOCl(g) will go down.

C) The temperature will go down.

D) There will be no effect on the equilibrium.



Answer A

The fact that the process of forming a solution is non-spontaneous means that it absorbs heat.

The fact that the process of forming a solution is non-spontaneous means that it absorbs heat.

Answer: True

For which of the reactions below does Kc (calculated using concentrations) equal KP (calculated using pressures)?

For which of the reactions below does Kc (calculated using concentrations) equal KP (calculated using pressures)?

A) N2(g) + O2(g) ←→2NO(g) Kp = 0.050

B) 2NO(g) + Cl2(g) ←→2NOCl(g) Kc = 4.6 x 104

C) 2SO3(g)←→2SO2(g) + O2(g) Kp = 16.5

D) 2SO3(g)←→2SO2(g) +O2(g) Kc = 0.230

Answer A

Calculate the Reaction Quotient (Q) for AgCl when 500 mL of 4 x 10-5M AgNO3(aq) is mixed with 500 mL of 3 x 10-5M NaCl(aq) and determine whether AgCl will precipitate.

Calculate the Reaction Quotient (Q) for AgCl when 500 mL of 4 x 10-5M AgNO3(aq) is mixed with 500 mL of 3 x 10-5M NaCl(aq) and determine whether AgCl will precipitate.

AgCl Solubility Product Ksp = 1.8 x 10-10


A) Q = 1.2 x 10-9; AgCl will not precipitate

B) Q = 1.2 x 10-9; AgCl will precipitate

C) Q = 3 x 10-10; AgCl will not precipitate

D) Q = 3 x 10-10; AgCl will precipitate


Answer A

METB is one of the compounds used as octane enhancers in unleaded gasoline. It is manufactured by the catalytic conversion of acetylene to benzene: 3C2H2(g) → C6H6(g). Which value of Kc would make this reaction most useful commercially?

METB is one of the compounds used as octane enhancers in unleaded gasoline. It is manufactured by the catalytic conversion of acetylene to benzene: 3C2H2(g) → C6H6(g). Which value of Kc would make this reaction most useful commercially?

A) Kc = 0.001

B) Kc = 1.00

C) Kc = 100


Answer C

Write the mathematical expression for the reaction quotient, Qc, for the following reaction:

Write the mathematical expression for the reaction quotient, Qc, for the following reaction:

2NH3(g) ←→N2(g) + 3H2(g)

A) Qc = (PN2 * P3H2) / (P3 NH3)

B) Qc = (PN2 * PH3) / PNH3

C) Qc = (P2 NH3) / (PN2 * P3 H2)

D) Qc = (PNH3) / (PN2 * PH2)

Answer A

Adding sodium cyanide to a saturated solution of AgCl(s) containing suspended AgCl will result in dissolving more AgCl since CN- forms a soluble complex with silver.

Adding sodium cyanide to a saturated solution of AgCl(s) containing suspended AgCl will result in dissolving more AgCl since CN- forms a soluble complex with silver.

Answer: True

Which of the following actions will decrease the amount of hydrazine gas (N2H4) produced in a closed container in the following reaction? Check all correct answers that apply.

Which of the following actions will decrease the amount of hydrazine gas (N2H4) produced in a closed container in the following reaction? Check all correct answers that apply.

N2(g) + 2H2(g) ←→N2H4(g) + heat ΔH = 95 kJ


A) decrease the temperature of the reaction

B) increase the temperature of the reaction

C) remove N2 from the reaction

D) increase the pressure of the reaction by decreasing the volume of the closed container



Answers: B, C, D

A reaction is considered to be at equilibrium when the concentration of products equals the concentration of reactants.

A reaction is considered to be at equilibrium when the concentration of products equals the concentration of reactants.

Answer: False

For which of the reactions would a change in pressure not shift the equilibrium concentration?

For which of the reactions would a change in pressure not shift the equilibrium concentration?

A) N2(g) + O2(g) ←→2NO(g) Kp = 2 x 10-2

B) P4(g) + 5O2(g) ←→P4O10(s) Kc = 0.05

C) CH4(g) + 2O2(g) ←→CO2(g) Kp = 6 x 103

D) Br2(g)←→2Br(g) Kp = 9 x 10-15


Answer: A

Lewis acid-base adducts (products) can be charged complexes or uncharged solids.

Lewis acid-base adducts (products) can be charged complexes or uncharged solids.

Answer: TRUE!

If a reaction is reversible, when can it be said to have reached equilibrium?

If a reaction is reversible, when can it be said to have reached equilibrium?

Answer: When a system has reached equilibrium, no further changes in the reactant and product concentrations occur.

Assuming that no equilibria other than dissolution is involved, calculate the concentration of iodide ions, [I-(aq)], in the following saturated solution of lead iodide, PbI2(s).

Assuming that no equilibria other than dissolution is involved, calculate the concentration of iodide ions, [I-(aq)], in the following saturated solution of lead iodide, PbI2(s).

Solubility product PbI2 Ksp = 9.8 x 10-9


A) [I-] = 0.0043M

B) [I-] = 9.8 x 10-9M

C) [I-] = 0.0013M

D) [I-] = 0.0026M


Answer D

According to LeChatelier's Principle which of the following will affect the equilibrium of the following reaction in a closed container? Check all correct answers that apply.

According to LeChatelier's Principle which of the following will affect the equilibrium of the following reaction in a closed container? Check all correct answers that apply.

Heat + 2NH3(g) ←→3H2(g) + N2(g) ΔH = +1200 kJ


A) Add nitrogen gas

B)Add hydrogen gas

C) Add ammonia gas

D) Add argon gas


Answer: All the Above

For which of the reactions below does Kc (calculated using concentrations) equal KP (calculated using pressures)?

For which of the reactions below does Kc (calculated using concentrations) equal KP (calculated using pressures)?

A)N2(g) + O2(g) ←→ 2NO(g) Kp = 2 x 10-2

B)P4(g) + 5O2(g) ←→P4O10(s) Kc = 0.05

C)CH4(g) + 2O2(g) ←→CO2(g) Kp = 6 x 103

D) Br2(g)←→2Br(g) Kp = 9 x 10-15

Answer A