Question 1

Which of the following compounds is an Arrhenius base?

Accepted Answer

A)  C6H12O6 
B)  HOCl 
C)  H2SO4 
D)  CH3NH2   
A)  C6H12O6 
B)  HOCl 
C)  H2SO4 
D)  CH3NH2

Question 2

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of MgSO3 and HI are mixed.

Accepted Answer

A)  2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g) 
B)  Mg2+(aq) + 2 I-(aq) → MgI2(s) 
C)  2 H+(aq) + SO32-(aq) + Mg2+(aq) + 2 I-(aq) → H2SO3(s) + MgI2(aq) 
D)  2 H+(aq) + SO32-(aq) + Mg2+(aq) + 2 I-(aq) → H2O(l) + SO2(g) + Mg2+(aq) + 2 I-(aq) 
E)  No reaction occurs. 
A)  2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g) 
B)  Mg2+(aq) + 2 I-(aq) → MgI2(s) 
C)  2 H+(aq) + SO32-(aq) + Mg2+(aq) + 2 I-(aq) → H2SO3(s) + MgI2(aq) 
D)  2 H+(aq) + SO32-(aq) + Mg2+(aq) + 2 I-(aq) → H2O(l) + SO2(g) + Mg2+(aq) + 2 I-(aq) 
E)  No reaction occurs.

Question 3

How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s)→ 2 K2O(s)+ 2 N2(g)+ 5 O2(g)

Accepted Answer

A)  0.290 mol N2 
B)  0.580 mol N2 
C)  18.5 mol N2 
D)  0.724 mol N2 
E)  1.73 mol N2 
A)  0.290 mol N2 
B)  0.580 mol N2 
C)  18.5 mol N2 
D)  0.724 mol N2 
E)  1.73 mol N2

Question 4

Define a spectator ion.

Accepted Answer

An ion tha

Question 5

Balance the chemical equation given below,and determine the number of grams of MgO that are needed to produce 20.0 g of Fe2O3. _____ MgO(s)+ _____ Fe(s)→ _____ Fe2O3(s)+ _____ Mg(s)

Accepted Answer

A)  0.0660 g 
B)  1.68 g 
C)  5.05 g 
D)  15.1 g 
A)  0.0660 g 
B)  1.68 g 
C)  5.05 g 
D)  15.1 g

Question 6

According to the following reaction,what amount of Al2S3 remains when 20.00 g of Al2S3 and 2.00 g of H2O are reacted? A few of the molar masses are as follows: Al2S3 = 150.17 g/mol,H2O = 18.02 g/mol. Al2S3(s)+ 6 H2O(l)→ 2 Al(OH)3(s)+ 3 H2S(g)

Accepted Answer

A)  28.33 g 
B)  14.00 g 
C)  8.33 g 
D)  19.78 g 
E)  17.22 g 
A)  28.33 g 
B)  14.00 g 
C)  8.33 g 
D)  19.78 g 
E)  17.22 g

Question 7

Determine the oxidation state of Ti in Ti(SO4)2.

Accepted Answer

A)  +2 
B)  +4 
C)  +6 
D)  0 
E)  -2 
A)  +2 
B)  +4 
C)  +6 
D)  0 
E)  -2

Question 8

How many milliliters of a 9.0 M H2SO4 solution are needed to make 0.25 L of a 3.5 M solution?

Accepted Answer

A)  0.097 mL 
B)  0.64 mL 
C)  97 mL 
D)  640 mL 
A)  0.097 mL 
B)  0.64 mL 
C)  97 mL 
D)  640 mL

Question 9

Match between columns
                        Premises: HS1U1B12S1U1B0SOS1U1B14S1U1B0(aq)+ 2 LiOH(aq)→ 2 HS1U1B12S1U1B0O(l)+ LiS1U1B12S1U1B0SO4(aq)
Mg(s)+ Cu(NOS1U1B13S1U1B0)S1U1B12S1U1B0(aq)→ Mg(NOS1U1B13S1U1B0)S1U1B12S1U1B0(aq)+ Cu(s)
NaCl(aq)+ AgNOS1U1B13S1U1B0(aq)→ AgCl(s)+ NaNOS1U1B13S1U1B0(aq)
HCl(aq)+ (NHS1U1B14S1U1B0)S1U1B12S1U1B0S(aq)→ HS1U1B12S1U1B0S(g)+ 2 NHS1U1B14S1U1B0Cl(aq)
CHS1U1B14S1U1B0(g)+ 2 OS1U1B12S1U1B0(g)→ COS1U1B12S1U1B0(g)+ 2 HS1U1B12S1U1B0O(g)

Accepted Answer

The Answer of combustion and gas evolution and precipitation and is...

Question 10

Give the percent yield when 28.16 g of CO2 are formed from the reaction of 8.000 moles of C8H18 with 4.000 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

Accepted Answer

A)  10.00% 
B)  12.50% 
C)  25.00% 
D)  6.250% 
E)  95.00 
A)  10.00% 
B)  12.50% 
C)  25.00% 
D)  6.250% 
E)  95.00

Question 11

Describe the difference between complete ionic and net ionic equations.

Accepted Answer

A complete ionic equation shows all of t

Question 12

Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction.A possibly useful molar mass is BCl3 = 117.16 g/mol. BCl3(g)+ 3 H2O(l)→ H3BO3(s)+ 3 HCl(g)

Accepted Answer

A)  75.9 g HCl 
B)  132 g HCl 
C)  187 g HCl 
D)  56.0 g HCl 
E)  25.3 g HCl 
A)  75.9 g HCl 
B)  132 g HCl 
C)  187 g HCl 
D)  56.0 g HCl 
E)  25.3 g HCl

Question 13

Which of the following solutions will have the highest concentration of chloride ions?

Accepted Answer

A)  0.60 M LiCl 
B)  0.40 M MgCl2 
C)  0.60 M AlCl3 
D)  0.40 M BaCl2 
E)  All of these solutions have the same concentration of chloride ions. 
A)  0.60 M LiCl 
B)  0.40 M MgCl2 
C)  0.60 M AlCl3 
D)  0.40 M BaCl2 
E)  All of these solutions have the same concentration of chloride ions.

Question 14

Identify the species reduced. 2 Al3+(aq)+ 2 Fe(s)→ 2 Al(s)+ 3 Fe2+(aq)

Accepted Answer

A)  Al3+ 
B)  Fe 
C)  Al 
D)  Fe2+ 
E)  This is not an oxidation-reduction reaction. 
A)  Al3+ 
B)  Fe 
C)  Al 
D)  Fe2+ 
E)  This is not an oxidation-reduction reaction.

Question 15

Sodium metal and water react to form hydrogen and sodium hydroxide.If 17.94 g of sodium react with water to form 0.78 g of hydrogen and 31.20 g of sodium hydroxide,what mass of water was involved in the reaction?

Accepted Answer

A)  14.04 g 
B)  17.94 g 
C)  30.42 g 
D)  31.98 g 
A)  14.04 g 
B)  17.94 g 
C)  30.42 g 
D)  31.98 g

Question 16

What element is undergoing oxidation (if any)in the following reaction? Zn(s)+ 2 AgNO3(aq)→ Zn(NO3)2(aq)+ 2 Ag(s)

Accepted Answer

A)  Zn 
B)  N 
C)  O 
D)  Ag 
E)  This is not an oxidation-reduction reaction. 
A)  Zn 
B)  N 
C)  O 
D)  Ag 
E)  This is not an oxidation-reduction reaction.

Question 17

When silver nitrate reacts with barium chloride,silver chloride and barium nitrate are formed.How many grams of silver chloride are formed when 10.2 g of silver nitrate reacts with 15.0 g of barium chloride?

Accepted Answer

A)  8.61 g 
B)  9.40 g 
C)  12.1 g 
D)  18.8 g 
A)  8.61 g 
B)  9.40 g 
C)  12.1 g 
D)  18.8 g

Question 18

What is the change in oxidation state for the manganese atom in the following unbalanced reduction half reaction? MnO4- (aq)+ H+(aq)→ Mn2+(aq)+ H2O(l)

Accepted Answer

A)  -7 
B)  -5 
C)  +5 
D)  +7 
A)  -7 
B)  -5 
C)  +5 
D)  +7

Question 19

Define an electrolyte.

Accepted Answer

A substance that dis

Question 20

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2 Mg(s)+ O2(g)→ 2 MgO(s)
How many moles of O2 are consumed when 2.10 mol of magnesium burns?

Accepted Answer

A)  0.0864 
B)  0.952 
C)  2.10 
D)  4.20 
E)  1.05 
A)  0.0864 
B)  0.952 
C)  2.10 
D)  4.20 
E)  1.05

Exam 4: Chemical Quantities and Aqueous Reactions

Which of the following compounds is an Arrhenius base?

Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of MgSO3 and HI are mixed.

How many moles of nitrogen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol. 4 KNO3(s)→ 2 K2O(s)+ 2 N2(g)+ 5 O2(g)

Define a spectator ion.

Balance the chemical equation given below,and determine the number of grams of MgO that are needed to produce 20.0 g of Fe2O3. _____ MgO(s)+ _____ Fe(s)→ _____ Fe2O3(s)+ _____ Mg(s)

According to the following reaction,what amount of Al2S3 remains when 20.00 g of Al2S3 and 2.00 g of H2O are reacted? A few of the molar masses are as follows: Al2S3 = 150.17 g/mol,H2O = 18.02 g/mol. Al2S3(s)+ 6 H2O(l)→ 2 Al(OH)3(s)+ 3 H2S(g)

Determine the oxidation state of Ti in Ti(SO4)2.

How many milliliters of a 9.0 M H2SO4 solution are needed to make 0.25 L of a 3.5 M solution?

Give the percent yield when 28.16 g of CO2 are formed from the reaction of 8.000 moles of C8H18 with 4.000 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O

Describe the difference between complete ionic and net ionic equations.

Determine the theoretical yield of HCl if 60.0 g of BCl3 and 37.5 g of H2O are reacted according to the following balanced reaction.A possibly useful molar mass is BCl3 = 117.16 g/mol. BCl3(g)+ 3 H2O(l)→ H3BO3(s)+ 3 HCl(g)

Which of the following solutions will have the highest concentration of chloride ions?

Identify the species reduced. 2 Al3+(aq)+ 2 Fe(s)→ 2 Al(s)+ 3 Fe2+(aq)

Sodium metal and water react to form hydrogen and sodium hydroxide.If 17.94 g of sodium react with water to form 0.78 g of hydrogen and 31.20 g of sodium hydroxide,what mass of water was involved in the reaction?

What element is undergoing oxidation (if any)in the following reaction? Zn(s)+ 2 AgNO3(aq)→ Zn(NO3)2(aq)+ 2 Ag(s)

When silver nitrate reacts with barium chloride,silver chloride and barium nitrate are formed.How many grams of silver chloride are formed when 10.2 g of silver nitrate reacts with 15.0 g of barium chloride?

What is the change in oxidation state for the manganese atom in the following unbalanced reduction half reaction? MnO4- (aq)+ H+(aq)→ Mn2+(aq)+ H2O(l)

Define an electrolyte.

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2 Mg(s)+ O2(g)→ 2 MgO(s) How many moles of O2 are consumed when 2.10 mol of magnesium burns?

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Give the net ionic equation for the reaction (if any)that occurs when aqueous solutions of MgSO₃ and HI are mixed.

How many moles of nitrogen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g/mol. 4 KNO₃(s)→ 2 K₂O(s)+ 2 N₂(g)+ 5 O₂(g)

Balance the chemical equation given below,and determine the number of grams of MgO that are needed to produce 20.0 g of Fe₂O₃. ___ MgO(s)+ _ Fe(s)→ _ Fe₂O₃(s)+ ___ Mg(s)

According to the following reaction,what amount of Al₂S₃ remains when 20.00 g of Al₂S₃ and 2.00 g of H₂O are reacted? A few of the molar masses are as follows: Al₂S₃= 150.17 g/mol,H₂O = 18.02 g/mol. Al₂S₃(s)+ 6 H₂O(l)→ 2 Al(OH)₃(s)+ 3 H₂S(g)

Determine the oxidation state of Ti in Ti(SO₄)₂.

How many milliliters of a 9.0 M H₂SO₄ solution are needed to make 0.25 L of a 3.5 M solution?

Give the percent yield when 28.16 g of CO₂ are formed from the reaction of 8.000 moles of C₈H₁₈ with 4.000 moles of O₂. 2 C₈H₁₈ + 25 O₂ → 16 CO₂ + 18 H₂O

Determine the theoretical yield of HCl if 60.0 g of BCl₃and 37.5 g of H₂O are reacted according to the following balanced reaction.A possibly useful molar mass is BCl₃ = 117.16 g/mol. BCl₃(g)+ 3 H₂O(l)→ H₃BO₃(s)+ 3 HCl(g)

Identify the species reduced. 2 Al³⁺(aq)+ 2 Fe(s)→ 2 Al(s)+ 3 Fe²⁺(aq)

What element is undergoing oxidation (if any)in the following reaction? Zn(s)+ 2 AgNO₃(aq)→ Zn(NO₃)₂(aq)+ 2 Ag(s)

What is the change in oxidation state for the manganese atom in the following unbalanced reduction half reaction? MnO₄^-(aq)+ H⁺(aq)→ Mn²⁺(aq)+ H₂O(l)

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2 Mg(s)+ O₂(g)→ 2 MgO(s) How many moles of O₂ are consumed when 2.10 mol of magnesium burns?