Question 1

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H2O? Assume an excess of KO. 4KO(s)+ 2H2O(l)→ 4KOH(s)+ O2(g)

Accepted Answer

A) 2.72 moles KOH 
B) 16.7 moles KOH 
C) 10.9 moles KOH 
D) 8.33 moles KOH 
E) 4.87 moles KOH

Question 2

Determine the oxidation state of Mn in KMnO₄.

Accepted Answer

The answer of Determine the oxidation state of Mn in...

Question 3

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g mol-1, HNO3 = 63.02 g mol-1. 3NO2(g)+ H2O(l)→ 2HNO3(aq)+ NO(g)

Accepted Answer

A) 38.0 g H2O 
B) 21.7 g H2O 
C) 43.4 g H2O 
D) 10.9 g H2O 
E) 26.5 g H2O

Question 4

How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g mol-1. 4KNO3(s)→ 2K2O(s)+ 2N2(g)+ 5O2(g)

Accepted Answer

A) 0.290 mol O2 
B) 0.580 mol O2 
C) 18.5 mol O2 
D) 0.724 mol O2 
E) 1.73 mol O2

Question 5

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl3. 2 ICl3 + 3H2O → ICl + HIO3 + 5HCl

Accepted Answer

A) 2.78 × 1024 molecules HCl 
B) 1.67 × 1024 molecules HCl 
C) 5.02 × 1025 molecules HCl 
D) 6.09 × 1025 molecules HCl 
E) 3.65 × 1024 molecules HCl

Question 6

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

Accepted Answer

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

Question 7

Aluminum metal reacts with aqueous iron(II)chloride to form aqueous aluminum chloride and iron metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients?

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4

Question 8

What is the oxidation number change for the bromine atom in the following unbalanced reduction half-reaction: Br O3- (aq)+ H+(aq)→ Br-(aq)+ H2O(l)

Accepted Answer

A) -7 
B) -6 
C) +6 
D) +7

Question 9

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s)+ N2(g)→ 2Li3N(s)
How many moles of lithium are needed to produce 0.60 mol of Li3N when the reaction is carried out in the presence of excess nitrogen?

Accepted Answer

A) 0.30 
B) 1.8 
C) 0.20 
D) 0.40 
E) 3.6

Question 10

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-1. BCl3(g)+ 3H2O(l)→ H3BO3(s)+ 3HCl(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

Question 11

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s)→ 2Na(s)+ 3N2(g)
How many grams of sodium azide are required to produce 33.0 g of nitrogen?

Accepted Answer

A) 1.77 
B) 0.785 
C) 76.6 
D) 51.1 
E) 114.9

Question 12

How many moles of BCl3 are needed to produce 10.0 g of HCl(aq)in the following reaction? BCl3(g)+ 3H2O(l)→ 3HCl(aq)+ B(OH)3(aq)

Accepted Answer

A) 0.0914 mol 
B) 0.274 mol 
C) 0.823 mol 
D) 10.9 mol

Question 13

Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride: Ag+(aq)+ Cl-(aq)→ AgCl(s)
Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.366 mol L-1 AgNO3 solution to completely precipitate the silver?

Accepted Answer

A) 9.15 × 10-3 g 
B) 1.57 × 10-4 g 
C) 0.535 g 
D) 0.157 g 
E) 6.39 × 103 g

Question 14

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s)+ O2(g)→ 2MgO(s)
How many moles of O2 are consumed when 0.770 mol of magnesium burns?

Accepted Answer

A) 0.0317 
B) 2.60 
C) 0.770 
D) 1.54 
E) 0.385

Question 15

Sodium metal and water react to form hydrogen and sodium hydroxide. If 5.98 g of sodium react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide, what mass of water was involved in the reaction?

Accepted Answer

A) 4.68 g 
B) 5.98 g 
C) 10.14 g 
D) 10.66 g

Question 16

Determine the reducing agent in the following reaction. 
2Li(s)+ Fe(C2H3O2)2(aq)→ 2LiC2H3O2(aq)+ Fe(s)

Accepted Answer

A) O 
B) H 
C) C 
D) Fe 
E) Li

Question 17

Which of the following describes NaCl?

Accepted Answer

A) weak acid 
B) weak electrolyte 
C) strong acid 
D) strong electrolyte 
E) nonelectrolyte

Question 18

Identify the oxidation state of H in HCl(aq).
 Mg(s)+ 2HCl(aq)→ MgCl2(aq)+ H2(g)

Accepted Answer

A) +1 
B) +2 
C) 0 
D) -1 
E) -2

Question 19

A stock solution of HNO3 is prepared and found to contain 13.5 mol L-1 of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, what is the concentration of the diluted solution?

Accepted Answer

A) 0.270 mol L-1 
B) 1.48 mol L-1 
C) 0.675 mol L-1 
D) 675 mol L-1 
E) 270 mol L-1

Question 20

Which pair of compounds is soluble in water?

Accepted Answer

A) HgBr2 and Hg2I2 
B) CuS and Na2S 
C) LiI and Ca(NO3)2 
D) K NO3 and CaCO3

Exam 4: Chemical Reactions and Stoichiometry

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H₂O? Assume an excess of KO. 4KO(s) + 2H₂O(l) → 4KOH(s) + O₂(g)

Determine the oxidation state of Mn in KMnO₄.

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO₃? Assume that there is excess NO₂ present. The molar masses are as follows: H₂O = 18.02 g mol^-1, HNO₃ = 63.02 g mol^-1. 3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g)

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g mol^-1. 4KNO₃(s) → 2K₂O(s) + 2N₂(g) + 5O₂(g)

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl₃. 2 ICl₃ + 3H₂O → ICl + HIO₃ + 5HCl

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

Aluminum metal reacts with aqueous iron(II) chloride to form aqueous aluminum chloride and iron metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients?

What is the oxidation number change for the bromine atom in the following unbalanced reduction half-reaction: BrO₃^-(aq) + H⁺(aq) → Br^-(aq) + H₂O(l)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N₂(g) → 2Li₃N(s) How many moles of lithium are needed to produce 0.60 mol of Li₃N when the reaction is carried out in the presence of excess nitrogen?

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^-1. BCl₃(g) + 3H₂O(l) → H₃BO₃(s) + 3HCl(g)

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN₃(s) → 2Na(s) + 3N₂(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?

How many moles of BCl₃ are needed to produce 10.0 g of HCl(aq) in the following reaction? BCl₃(g) + 3H₂O(l) → 3HCl(aq) + B(OH) ₃(aq)

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O₂(g) → 2MgO(s) How many moles of O₂ are consumed when 0.770 mol of magnesium burns?

Sodium metal and water react to form hydrogen and sodium hydroxide. If 5.98 g of sodium react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide, what mass of water was involved in the reaction?

Determine the reducing agent in the following reaction. 2Li(s) + Fe(C₂H₃O₂) ₂(aq) → 2LiC₂H₃O₂(aq) + Fe(s)

Which of the following describes NaCl?

Identify the oxidation state of H in HCl(aq) . Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)

A stock solution of HNO₃ is prepared and found to contain 13.5 mol L^-1 of HNO₃. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, what is the concentration of the diluted solution?

Which pair of compounds is soluble in water?

Exam 4: Chemical Reactions and Stoichiometry

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H2O? Assume an excess of KO. 4KO(s) + 2H2O(l) → 4KOH(s) + O2(g)

Determine the oxidation state of Mn in KMnO4.

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g mol-1, HNO3 = 63.02 g mol-1. 3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g)

How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g mol-1. 4KNO3(s) → 2K2O(s) + 2N2(g) + 5O2(g)

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl3. 2 ICl3 + 3H2O → ICl + HIO3 + 5HCl

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

Aluminum metal reacts with aqueous iron(II) chloride to form aqueous aluminum chloride and iron metal. What is the stoichiometric coefficient for aluminum when the chemical equation is balanced using the lowest, whole-number stoichiometric coefficients?

What is the oxidation number change for the bromine atom in the following unbalanced reduction half-reaction: Br O3- (aq) + H+(aq) → Br-(aq) + H2O(l)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) How many moles of lithium are needed to produce 0.60 mol of Li3N when the reaction is carried out in the presence of excess nitrogen?

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-1. BCl3(g) + 3H2O(l) → H3BO3(s) + 3HCl(g)

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s) → 2Na(s) + 3N2(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?

How many moles of BCl3 are needed to produce 10.0 g of HCl(aq) in the following reaction? BCl3(g) + 3H2O(l) → 3HCl(aq) + B(OH) 3(aq)

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O2(g) → 2MgO(s) How many moles of O2 are consumed when 0.770 mol of magnesium burns?

Sodium metal and water react to form hydrogen and sodium hydroxide. If 5.98 g of sodium react with water to form 0.26 g of hydrogen and 10.40 g of sodium hydroxide, what mass of water was involved in the reaction?

Determine the reducing agent in the following reaction. 2Li(s) + Fe(C2H3O2) 2(aq) → 2LiC2H3O2(aq) + Fe(s)

Which of the following describes NaCl?

Identify the oxidation state of H in HCl(aq) . Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)

A stock solution of HNO3 is prepared and found to contain 13.5 mol L-1 of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, what is the concentration of the diluted solution?

Which pair of compounds is soluble in water?

According to the following balanced reaction, how many moles of KOH will be formed from 5.44 moles of H₂O? Assume an excess of KO. 4KO(s) + 2H₂O(l) → 4KOH(s) + O₂(g)

Determine the oxidation state of Mn in KMnO₄.

Consider the following balanced reaction. How many grams of water are required to form 75.9 g of HNO₃? Assume that there is excess NO₂ present. The molar masses are as follows: H₂O = 18.02 g mol^-1, HNO₃ = 63.02 g mol^-1. 3NO₂(g) + H₂O(l) → 2HNO₃(aq) + NO(g)

How many moles of oxygen are formed when 58.6 g of KNO₃ decomposes according to the following reaction? The molar mass of KNO₃ is 101.11 g mol^-1. 4KNO₃(s) → 2K₂O(s) + 2N₂(g) + 5O₂(g)

How many molecules of HCl are formed when 50.0 g of water reacts according to the following balanced reaction? Assume excess ICl₃. 2 ICl₃ + 3H₂O → ICl + HIO₃ + 5HCl

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

What is the oxidation number change for the bromine atom in the following unbalanced reduction half-reaction: BrO₃^-(aq) + H⁺(aq) → Br^-(aq) + H₂O(l)

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N₂(g) → 2Li₃N(s) How many moles of lithium are needed to produce 0.60 mol of Li₃N when the reaction is carried out in the presence of excess nitrogen?

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^-1. BCl₃(g) + 3H₂O(l) → H₃BO₃(s) + 3HCl(g)

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN₃(s) → 2Na(s) + 3N₂(g) How many grams of sodium azide are required to produce 33.0 g of nitrogen?

How many moles of BCl₃ are needed to produce 10.0 g of HCl(aq) in the following reaction? BCl₃(g) + 3H₂O(l) → 3HCl(aq) + B(OH) ₃(aq)

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O₂(g) → 2MgO(s) How many moles of O₂ are consumed when 0.770 mol of magnesium burns?

Determine the reducing agent in the following reaction. 2Li(s) + Fe(C₂H₃O₂) ₂(aq) → 2LiC₂H₃O₂(aq) + Fe(s)

Identify the oxidation state of H in HCl(aq) . Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g)

A stock solution of HNO₃ is prepared and found to contain 13.5 mol L^-1 of HNO₃. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, what is the concentration of the diluted solution?