Chapter 4

CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) A) combustion B) acid base C) oxidation reduction D) gas evolution E) precipitation

A

Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution. A) 1.50 M B) 1.18 M C) 0.130 M D) 0.768 M E) 2.30 M

A) 1.50 M

When silver nitrate reacts with barium chloride, silver chloride and barium nitrate are formed. How many grams of silver chloride are formed when 10.0 g of silver nitrate reacts with 15.0 g of barium chloride? A) 8.44 g B) 9.40 g C) 11.9 g D) 18.8 g

A) 8.44 g

Which of the following compounds is insoluble in water? A) Hg2I2 B) MgSO4 C) (NH4)2CO3 D) BaS E) All of these compounds are soluble in water.

A) Hg2I2

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

B) -6

Mg(s) + Cu(NO3)2(aq) → Mg(NO3)2(aq) + Cu(s) A) combustion B) acid base C) oxidation reduction D) gas evolution E) precipitation

C

What mass, in g, of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl2 solution? 2 AgC2H3O2(aq) + MgCl2(aq) → 2 AgCl(s) + Mg(C2H3O2)2(aq) A) 0.838 g B) 1.72 g C) 0.859 g D) 2.56 g E) 1.70 g

A) 0.838 g

According to the balanced equation shown below, 4.00 moles of oxalic acid, H2C2O4, reacts with ________ moles of permanganate, MnO4-. 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + Mn2+(aq) + 8 H2O(l) A) 1.60 B) 4.00 C) 8.00 D) 9.00

A) 1.60

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

A) 4.68 g

Determine the oxidation state of Mn in KMnO4.

Answer: +7

How many moles of CO2+ are present in 0.150 L of a 0.200 M solution of CoI2?

Answer: 0.0300

Calculate the concentration (M) of sodium ions in a solution made by diluting 40.0 mL of a 0.474 M solution of sodium sulfide to a total volume of 300 mL.

Answer: 0.126

What is the concentration (M) of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient water to give 425 mL of solution?

Answer: 0.29

What is the concentration (M) of sodium ions in 4.57 L of a .398 M Na3P solution?

Answer: 1.19

There are ________ mol of bromide ions in 0.900 L of a 0.500M solution of AlBr3.

Answer: 1.35

How many grams of H3PO4 are in 265 mL of a 1.50 M solution of H3PO4?

Answer: 39.0

How many grams of CH3OH must be added to water to prepare 150mL of a solution that is 2.0 M CH3OH?

Answer: 9.6

What is the oxidation number of the oxygen atom in Rb2O2? A) -2 B) -1 C) +1 D) +2

B) -1

If 100. mL of 0.400 M Na2SO4 is added to 200. mL of 0.600 M NaCl, what is the concentration of Na+ ions in the final solution? Assume that the volumes are additive. A) 0.534 M B) 0.667 M C) 1.00 M D) 1.40 M

B) 0.667 M

According to the following balanced reaction, how many moles of KO are required to exactly react with 5.44 moles of H2O? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g) A) 5.44 moles H2O B) 10.9 moles H2O C) 21.8 moles H2O D) 2.72 moles H2O E) 1.36 moles H2O

B) 10.9 moles H2O

How many milliliters of a 0.266 M LiNO3 solution are required to make 150.0 mL of 0.075 M LiNO3 solution? A) 53.2 mL B) 42.3 mL C) 18.8 mL D) 23.6 mL E) 35.1 mL

B) 42.3 mL

Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 2Mg(s) + O2(g) → 2MgO(s) When 4.00 g of magnesium burns, the theoretical yield of magnesium oxide is ________ g. A) 4.00 B) 6.63 C) 0.165 D) 3.32 E) 13.3

B) 6.63

Identify the spectator ions in the following molecular equation. KBr(aq) + AgNO3(aq) → AgBr(s) + KNO3(aq) A) Ag+ & Br- B) K+ & NO3- C) K+ & Br- D) Ag+ & NO3- E) There are no spectator ions in this reaction.

B) K+ & NO3-

A stock solution of HNO3 is prepared and found to contain 13.5 M of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M. A) 0.270 B) 1.48 C) 0.675 D) 675 E) 270

C) 0.675

Based on the balanced chemical equation shown below, determine the molarity of a solution containing Fe2+(aq), if 40.00 mL of the Fe2+(aq) solution is required to completely react with 30.00 mL of a 0.250 M potassium bromate, KBrO3(aq), solution. The chemical equation for the reaction is 6 Fe2+(aq) + BrO3-(aq) + 6 H+(aq) → 6 Fe3+(aq) + Br-(aq) + 3 H2O(l). A) 0.0312 M B) 0.188 M C) 1.12 M D) 2.00 M

C) 1.12 M

According to the following balanced reaction, how many moles of KO are required to exactly react with 5.44 moles of H2O? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g) A) 2.72 moles H2O B) 16.7 moles H2O C) 10.9 moles H2O D) 8.33 moles H2O E) 4.87 moles H2O

C) 10.9 moles H2O

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed. A) 2 H+(aq) + CO32-(aq) → H2CO3(s) B) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 NaCl(aq) C) 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g) D) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl-(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq) E) No reaction occurs.

C) 2 H+(aq) + CO32-(aq) → H2O(l) + CO2(g)

Which of the following is a precipitation reaction? A) Zn(s) + 2 AgNO3(aq) → 2 Ag(s) + Zn(NO3)2(aq) B) NaCl(aq) + LiI(aq) → NaI(aq) + LiCl(aq) C) 2 LiI(aq) + Hg2(NO3)2(aq) → Hg2I2(s) + 2 LiNO3(aq) D) HCl(aq) + KOH(aq) → KCl(aq) + H2O(l) E) None of the above are precipitation reactions.

C) 2 LiI(aq) + Hg2(NO3)2(aq) → Hg2I2(s) + 2 LiNO3(aq)

How many chloride ions are present in 65.5 mL of 0.210 M AlCl3 solution? A) 4.02 × 1023 chloride ions B) 5.79 × 1024 chloride ions C) 2.48 × 1022 chloride ions D) 8.28 × 1021 chloride ions E) 1.21 × 1022 chloride ions

C) 2.48 × 1022 chloride ions

How many grams of AgNO3 are needed to make 250. mL of a solution that is 0.135 M? A) 0.0917 g B) 0.174 g C) 5.73 g D) 91.7 g

C) 5.73 g

How many milliliters of 0.550 M hydriodic acid are needed to react with 15.00 mL of 0.217 M CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H2O(l) A) 0.0263 mL B) 0.169 mL C) 5.92 mL D) 38.0 mL

C) 5.92 mL

Which of the following is not a strong electrolyte? A) LiOH B) CaCl2 C) MgCO3 D) NaC2H3O2 E) Li2SO4

C) MgCO3

What are the spectator ions for the following reaction in aqueous solution: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) A) Ag+ B) Cl- C) Na+ & NO3- D) Na+ & Cl-

C) Na+ & NO3-

Which pair of compounds is soluble in water? A) Ag Cl and AgBr B) CoS and K2S C) NaI and Cu(NO3)2 D) NH4NO3 and BaCO3

C) NaI and Cu(NO3)2

Which substance is the limiting reactant when 2.0 g of sulfur reacts with 3.0 g of oxygen and 4.0 g of sodium hydroxide according to the following chemical equation: 2 S(s) + 3 O2(g) + 4 NaOH(aq) → 2 Na2SO4(aq) + 2 H2O(l) A) S(s) B) O2(g) C) NaOH(aq) D) None of these substances is the limiting reactant.

C) NaOH(aq)

Which one of the following compounds is insoluble in water? A) Ca Cl2 B) NaNO3 C) Pb Cl2 D) K2CO3

C) Pb Cl2

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

D) 51.1

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

D) 56.0 g HCl

What volume (in mL) of 0.0887 M MgF2 solution is needed to make 275.0 mL of 0.0224 M MgF2 solution? A) 72.3 mL B) 91.8 mL C) 10.9 mL D) 69.4 mL E) 14.4 mL

D) 69.4 mL

Balance the chemical equation given below, and determine the number of grams of MgO are needed to produce 10.0 g of Fe2O3 . ____ MgO(s) + ____ Fe(s) → ____ Fe2O3(s) +_____ Mg(s) A) 0.312 g B) 0.841 g C) 2.52 g D) 7.57 g

D) 7.57 g

How many aluminum ions are present in 65.5 mL of 0.210 M AlF3 solution? A) 4.02 × 1023 aluminum ions B) 5.79 × 1024 aluminum ions C) 2.48 × 1022 aluminum ions D) 8.28 × 1021 aluminum ions E) 1.21 × 1022 aluminum ions

D) 8.28 × 1021 aluminum ions

Which of the following compounds is an Arrhenius base? A) C6H12O6 B) HOCl C) H2SO4 D) C6H5NH2

D) C6H5NH2

Which of the following pairs of aqueous solutions will produce a precipitate when mixed? A) HCl + LiOH B) Li2S + HCl C) K2CO3 + HNO3 D) MgCl2 + KOH E) All of these solution pairs will produce a precipitate.

E) All of these solution pairs will produce a precipitate.

A student prepared a stock solution by dissolving 10.0 g of KOH in enough water to make 150. mL of solution. She then took 15.0 mL of the stock solution and diluted it with enough water to make water to make 65.0 mL of a final solution. What is the concentration of KOH for the final solution? A) 0.274 M B) 0.356 M C) 2.81 M D) 3.65 M

A) 0.274 M

Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s) A) Ag B) Ni C) Cl D) O E) This is not an oxidation-reduction reaction.

A) Ag

What precipitate is most likely formed from a solution containing Ba+2, Na+1, OH-1, and CO3-2. A) NaOH B) BaCO3 C) Na2CO3 D) Ba(OH)2

B) BaCO3

Which substance is oxidized in the following reaction? 5C2O42- + 2MnO4- + 16H+ → 10 CO2 + 2Mn2+ + 4H2O) A) 2MnO4- B) C2O42- C) H+ D) none

B) C2O42-

Which of the following compounds is not an Arrhenius acid? A) CH3CO2H B) CH3CH2NH2 C) HNO2 D) H2SO4

B) CH3CH2NH2

Which of the compounds of H2C2O4, Ca(OH)2, KOH, and HI, behave as acids when they are dissolved in water? A) Ca(OH)2 and KOH B) H2C2O4 and HI C) only HI D) only KOH

B) H2C2O4 and HI

How many H+ ions can the acid, H2SO4, donate per molecule? A) 0 B) 1 C) 2 D) 3

C) 2

Which one of the following compounds behaves as an acid when dissolved in water? A) RaO B) C4H10 C) HI D) RbOH

C) HI

What is the concentration of NO3- ions in a solution prepared by dissolving 25.0 g of Ca(NO3)2 in enough water to produce 300. mL of solution? A) 0.254 M B) 0.508 M C) 0.672 M D) 1.02 M

D) 1.02 M

NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) A) combustion B) acid base C) oxidation reduction D) gas evolution E) precipitation

E

Determine the oxidation state of Cl in NaClO3. A) +6 B) +4 C) +3 D) +2 E) +5

E) +5

Lithium and nitrogen react to produce lithium nitride by the following reaction. 6Li(s) + N2(g) → 2Li3N(s) How many moles of N2 are needed to react with 0.500 mol of lithium? A) 3.00 B) 0.500 C) 0.167 D) 1.50 E) 0.0833

E) 0.0833

A solution is prepared by mixing 50.0 mL of 0.100 M HCl and 10.0 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution? A) 0.183 B) 8.57 C) 3.50 D) 0.0500 E) 0.117

E) 0.117

How many moles of LiI are contained in 258.6 mL of 0.0296 M LiI solution? A) 1.31 × 10-3 mol B) 8.74 × 10-3 mol C) 1.14 × 10-3 mol D) 3.67 × 10-3 mol E) 7.65 × 10-3 mol

E) 7.65 × 10-3 mol

Determine the percent yield of a reaction that produces 28.65 g of Fe when 50.00 g of Fe2O3 react with excess Al according to the following reaction. Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s) A) 61.03% B) 28.65% C) 57.30% D) 20.02% E) 81.93%

E) 81.93%

How many grams of Li3N can be formed from 1.75 moles of Li? Assume an excess of nitrogen. 6 Li(s) + N2(g) → 2 Li3N(s) A) 18.3 g Li3N B) 20.3 g Li3N C) 58.3 g Li3N D) 61.0 g Li3N E) 15.1 g Li3N

B) 20.3 g Li3N

What is the oxidation number of the sulfur atom in Li2SO4? A) -2 B) +2 C) +4 D) +6

D) +6

What element is undergoing reduction (if any) in the following reaction? Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s) A) Zn B) N C) O D) Ag E) This is not an oxidation-reduction reaction.

D) Ag

Determine the oxidation state of P in PO33-. A) +3 B) +6 C) +2 D) 0 E) -3

A) +3

Give the oxidation state for S in SO3-2. A) +4 B) +6 C) -2 D) +2 E) +5

A) +4

How many grams of CaCl2 are formed when 15.00 mL of 0.00237 M Ca(OH)2 reacts with excess Cl2 gas? 2 Ca(OH)2(aq) + 2 Cl2(g) → Ca(OCl)2(aq) + CaCl2(s) + 2 H2O(l) A) 0.00197 g B) 0.00394 g C) 0.00789 g D) 0.0507 g

A) 0.00197 g

Which of the following solutions will have the highest electrical conductivity? A) 0.045 M Al2(SO4)3 B) 0.050 M (NH4)2CO3 C) 0.10 M LiBr D) 0.10 M NaI E) 0.10 M KF

A) 0.045 M Al2(SO4)3

What is the molarity of a potassium triiodide solution, KI3(aq), if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.200 M thiosulfate solution, K2S2O3(aq)? The chemical equation for the reaction is 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq). A) 0.0833 M B) 0.120 M C) 0.167 M D) 0.333 M

A) 0.0833 M

How many moles of BCl3 are needed to produce 10.0 g of HCl(aq) in the following reaction? BCl3(g) + 3 H2O(l) → 3 HCl(aq) + B(OH)3(aq) A) 0.0914 mol B) 0.274 mol C) 0.823 mol D) 10.9 mol

A) 0.0914 mol

Lithium and nitrogen react to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) How many moles of lithium nitride are produced when 0.450 mol of lithium react in the presence of excess nitrogen? A) 0.150 B) 0.900 C) 0.0750 D) 1.35 E) 0.225

A) 0.150

In an acid-base neutralization reaction 38.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution? A) 0.194 M B) 0.387 M C) 0.775 M D) 1.29 M

A) 0.194 M

1.06g of Na2CO3 is dissolved in 100mL of water. What is the molarity of Na+ ions in the solution? A) 0.2 M B) 0.1 M C) 1 × 10-4 M D) 0.01 M

A) 0.2 M

The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)? A) 0.20 M B) 0.40 M C) 0.10 M D) 0.36 M E) 0.25 M

A) 0.20 M

Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO2(g) + H2O(l) → HNO3(l) + NO(g) Suppose that 4mol NO2 and 2 H2O mol combine and react completely. How many moles of the reactant in excess are present after the reaction has completed? A) 0.7 B) 1 C) 0 D) 3

A) 0.7

A solution is prepared by adding 1.60 g of solid NaCl to 50.0 mL of 0.100 M CaCl2. What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL. A) 0.747 B) 0.647 C) 0.132 D) 0.232 E) 0.547

A) 0.747

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution? A) 0.801 B) 0.315 C) 0.629 D) 125 E) 0.400

A) 0.801

When 31.2 mL of 0.500 M AgNO3 is added to 25.0 mL of 0.300 M NH4Cl, how many grams of AgCl are formed? AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4NO3(aq) A) 1.07 g B) 2.24 g C) 3.31 g D) 6.44 g

A) 1.07 g

When 7.00 × 1022 molecules of ammonia react with 6.00 × 1022 molecules of oxygen according to the chemical equation shown below, how many grams of nitrogen gas are produced? 4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g) A) 1.63 g B) 1.86 g C) 4.19 g D) 6.51 g

A) 1.63 g

Give the theoretical yield, in grams, of CO2 from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O A) 112.7 g B) 102.4 g C) 176.0 g D) 704.0 g

A) 112.7 g

A 14.01 g sample of N2 reacts with 3.02 g of H2 to form ammonia (NH3). If ammonia is the only product, what mass of ammonia is formed? A) 17.01 g B) 1.10 g C) 14.01 g D) 3.02 g E) 23.07 g

A) 17.01 g

What are the coefficients in front of NO3-(aq) and Cu(s) when the following redox equation is balanced in an acidic solution: ____ NO3-(aq) + ____ Cu(s) → ____ NO(g) + ____ Cu2+(aq)? A) 2, 3 B) 2, 6 C) 3, 4 D) 3, 6

A) 2, 3

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 + 3 H2O → ICl + HIO3 + 5 HCl 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

A) 2.78 × 1024 molecules HCl

According to the following balanced reaction, how many moles of NO are formed from 8.44 moles of NO2 if there is plenty of water present? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) A) 2.81 moles NO B) 25.3 moles NO C) 8.44 moles NO D) 5.50 moles NO E) 1.83 moles NO

A) 2.81 moles NO

What is the concentration of an AlCl3 solution if 150. mL of the solution contains 450. mg of Cl- ion? A) 2.82 × 10-2 M B) 6.75 × 10-2 M C) 8.46 × 10-2 M D) 2.54 × 10-1 M

A) 2.82 × 10-2 M

How many milliliters of 0.260 M Na2S are needed to react with 40.00 mL of 0.315 M AgNO3? Na2S(aq) + 2 AgNO3(aq) → 2 NaNO3(aq) + Ag2S(s) A) 24.2 mL B) 48.5 mL C) 66.0 mL D) 96.9 mL

A) 24.2 mL

If the percent yield for the following reaction is 75.0%, and 45.0 g of NO2 are consumed in the reaction, how many grams of nitric acid, HNO3(aq) are produced? 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) A) 30.8 g B) 41.1 g C) 54.8 g D) 69.3 g

A) 30.8 g

How many moles of CH3CH2OH are contained in 548 mL of 0.0788 M CH3CH2OH solution? A) 4.32 × 10-2 mol B) 2.32 × 10-2 mol C) 6.95 × 10-2 mol D) 1.44 × 10-2 mol E) 5.26 × 10-2 mol

A) 4.32 × 10-2 mol

Carbonic acid can form water and carbon dioxide upon heating. How much carbon dioxide is formed from 6.20 g of carbonic acid? H2CO3 → H2O + CO2 A) 4.40 g B) 8.80 g C) 2.20 g D) 6.20 g

A) 4.40 g

Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L. ____ NH3(g) + ____ O2(g) → ____ NO(g) + ____ H2O(l) A) 7.32 L B) 11.1 L C) 11.5 L D) 17.3 L

A) 7.32 L

According to the following reaction, how many grams of sulfur are formed when 37.4 g of water are formed? 2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l) A) 99.8 g S B) 66.6 g S C) 56.1 g S D) 44.4 g S E) 14.0 g S

A) 99.8 g S

Choose the statement below that is true. A) A weak acid solution consists of mostly nonionized acid molecules. B) The term "strong electrolyte" means that the substance is extremely reactive. C) A strong acid solution consists of only partially ionized acid molecules. D) The term "weak electrolyte" means that the substance is inert. E) A molecular compound that does not ionize in solution is considered a strong electrolyte.

A) A weak acid solution consists of mostly nonionized acid molecules.

What reagent could be used to separate Br- from CH3CO2- when added to an aqueous solution containing both? A) AgNO3(aq) B) Ba(OH)2(aq) C) CuSO4(aq) D) NaI(aq)

A) AgNO3(aq)

What reagent could not be used to separate Br- from CO32- when added to an aqueous solution containing both? A) AgNO3(aq) B) Ca(NO3)2(aq) C) Cu(NO3)2(aq) D) Fe(NO3)2(aq)

A) AgNO3(aq)

The mixing of which pair of reactants will result in a precipitation reaction? A) Ba(NO3)2(aq) + Na2CO3(aq) B) K2SO4(aq) + Cu(NO3)2(aq) C) NaClO4(aq) + (NH4)2S(aq) D) NH4Br(aq) + NH4I(aq)

A) Ba(NO3)2(aq) + Na2CO3(aq)

Choose the reaction that represents the combustion of C6H12O2. A) C6H12O2(l) + 8 O2(g) → 6 CO2(g) + 6 H2O(g) B) Mg(s) + C6H12O2(l) → MgC6H12O2(aq) C) 6 C(s) + 6 H2(g) + O2(g) → C6H12O2(l) D) C6H12O2(l) → 6 C(s) + 6 H2(g) + O2(g) E) None of the above represent the combustion of C6H12O2.

A) C6H12O2(l) + 8 O2(g) → 6 CO2(g) + 6 H2O(g)

Which of the compounds H2C2O4, Ca(OH)2, KOH, and HI, behave as bases when they are dissolved in water? A) Ca(OH)2 and KOH B) H2C2O4 and HI C) only HI D) only KOH

A) Ca(OH)2 and KOH

Which of the following compounds is soluble in water? A) CaS B) MgCO3 C) PbCl2 D) BaSO4 E) None of these compounds is soluble in water.

A) CaS

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4 and KOH are mixed. A) H+(aq) + OH-(aq) → H2O(l) B) 2 K+(aq) + SO42-(aq) → K2SO4(s) C) H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H2O(l) + K2SO4(s) D) H22+(aq) + OH-(aq) → H2(OH)2(l) E) No reaction occurs.

A) H+(aq) + OH-(aq) → H2O(l)

Which of the following is considered a strong electrolyte? A) NH4NO3 B) C12H22O11 C) PbCl2 D) HC2H3O2 E) CH3OH

A) NH4NO3

If 294 grams of FeS2 is allowed to react with 176 grams of O2 according to the following unbalanced equation, how many grams of Fe2O3 are produced? FeS2 + O2 → Fe2O3 + SO2

Answer: 160

What is the concentration (M) of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in sufficient water to give exactly 230 mL of solution?

Answer: 2.28

How many grams of NaOH (MW = 40.0) are there in 250.0 mL of a 0.275 M NaOH solution?

Answer: 2.75

Describe the difference between complete ionic and net ionic equations.

Answer: A complete ionic equation shows all of the substances present in the reaction mixture. A net ionic equation only shows the substances that are participating in the reaction. The spectator ions are absent in the net ionic equation.

Define a net ionic equation.

Answer: A net ionic equation is an equation showing only the species that actually change during the reaction.

What causes a precipitation reaction to occur between two soluble compounds?

Answer: A precipitate, or insoluble compound, forms from a pair of the ions present that participate in a reaction. This "traps" some of the ions into a newly formed compound causing reaction.

Explain the difference between a strong and weak electrolyte. Give an example of each

Answer: A strong electrolyte is either an ionic compound that is soluble in water or a molecular compound that ionizes completely in water. Possible examples are NaCl or HCl. A weak electrolyte is only slightly soluble or does not ionize to any great extent in water. Possible examples are AgCl or HC2H3O2.

Define a strong electrolyte.

Answer: A substance that dissolves in water to form a solution that conducts electricity.

How can you tell if a reaction is an oxidation-reduction reaction?

Answer: At least one species is losing electrons while at least one other species is gaining electrons. This can be evaluated by assigning oxidation numbers to each element present and looking to see if these change from reactant to product.

List the spectator ions in the following reaction. Ba+2(aq) + 2 OH-(aq) + 2 Na +(aq) + CO3-2(aq) → 2 Na +(aq) + 2 OH-(aq) + BaCO3(s)

Answer: Na+ and OH-

How would the concentration change if a 1.0 L flask of 1.0 M NaCl were left uncapped on a laboratory bench for several days. Why?

Answer: The concentration would slowly increase as water from the solution evaporated. This is because the amount of NaCl in the flask would remain constant while the amount of water decreases.

H2SO4(aq) + 2 LiOH(aq) → 2 H2O(l) + Li2SO4(aq) A) combustion B) acid base C) oxidation reduction D) gas evolution E) precipitation

B

Determine the oxidation state of Sn in Sn(SO4)2. A) +2 B) +4 C) +6 D) 0 E) -2

B) +4

Determine the molarity of a solution formed by dissolving 468 mg of MgI2 in enough water to yield 50.0 mL of solution. A) 0.0297 M B) 0.0337 M C) 0.0936 M D) 0.0107 M E) 0.0651 M

B) 0.0337 M

What is the concentration of FeCl3 in a solution prepared by dissolving 20.0 g of FeCl3 in enough water to make 275 mL of solution? A) 4.48 × 10-4 M B) 0.448 M C) 2.23 M D) 2.23 × 103 M

B) 0.448 M

What volume of a 0.540 M NaOH solution contains 11.5 g of NaOH? A) 0.155 L B) 0.532 L C) 1.88 L D) 6.44 L

B) 0.532 L

How many moles of NaCl are required to make 250 mL of a 3.00 M solution? A) 750 moles B) 0.750 moles C) 3 moles D) 0.250 moles

B) 0.750 moles

How many grams of calcium chloride are needed to produce 1.50 g of potassium chloride? CaCl2(aq) + K2CO3(aq) → 2 KCl(aq) + CaCO3(aq) A) 0.896 g B) 1.12 g C) 2.23 g D) 4.47 g

B) 1.12 g

How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in 14.3 mL of 0.140 M sucrose solution? A) 8.29 × 1022 molecules C12H22O11 B) 1.21 × 1021 molecules C12H22O11 C) 6.15 × 1022 molecules C12H22O11 D) 1.63 × 1023 molecules C12H22O11 E) 5.90 × 1024 molecules C12H22O11

B) 1.21 × 1021 molecules C12H22O11

Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO2(g) + H2O(l) → HNO3(l) + NO(g) Suppose that 4 mol NO2 and 2 H2O mol combine and react completely. How many moles of NO are produced after the reaction has completed? A) 2 B) 1.33 C) 3 D) 4

B) 1.33

Balance the chemical equation given below, and determine the number of moles of iodine that reacts with 30.0 g of aluminum. ____ Al(s) + ____ I2(s) → ____ Al2I6(s) A) 0.741 mol B) 1.67 mol C) 2.22 mol D) 3.33 mol

B) 1.67 mol

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

B) 1.8

Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 45.00 mL of 0.00150 M calcium hydroxide. ____ Ca(OH)2(aq) + ____ H3PO4(aq) → ____ Ca3(PO4)2(aq) + ____ H2O(l) A) 3.04 mL B) 15.0 mL C) 22.5 mL D) 33.8 mL

B) 15.0 mL

Which of the following is an acid base reaction? A) C(s) + O2(g) → CO2(g) B) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq) C) Fe(s) + 2 AgNO3(aq) → 2 Ag(s) + Fe(NO3)2(aq) D) MgSO4(aq) + Ba(NO3)2(aq) → Mg(NO3)2(aq) + BaSO4(s) E) None of the above are acid base reactions.

B) 2 HClO4(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(ClO4)2(aq)

How many milliliters of a stock solution of 11.1 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3? A) 0.0444 mL B) 22.5 mL C) 2.78 mL D) 44.4 mL E) 0.0225 mL

B) 22.5 mL

When 11.0 g of calcium metal is reacted with water, 5.00 g of calcium hydroxide is produced. Using the following balanced equation, calculate the percent yield for the reaction? Ca(s) + 2 H2O(l) → Ca(OH)2(aq) + H2(g) A) 12.3% B) 24.6% C) 45.5% D) 84.0%

B) 24.6%

Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 4.000 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O A) 20.00% B) 25.00% C) 88.90% D) 22.20%

B) 25.00%

A FeCl3 solution is 0.175 M. How many mL of a 0.175 M FeCl3 solution are needed to make 450. mL of a solution that is 0.300 M in Cl- ion? A) 0.771 mL B) 257 mL C) 771 mL D) It is not possible to make a more concentrated solution from a less concentrated solution.

B) 257 mL

Consider the following reaction. How many moles of oxygen are required to produce 2.33 moles of water? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g) A) 1.55 moles O2 B) 3.50 moles O2 C) 2.33 moles O2 D) 4.14 moles O2 E) 6.21 moles O2

B) 3.50 moles O2

According to the following reaction, what mass of PbCl2 can form from 235 mL of 0.110 M KCl solution? Assume that there is excess Pb(NO3)2. 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) A) 7.19 g B) 3.59 g C) 1.80 g D) 5.94 g E) 1.30 g

B) 3.59 g

Dinitrogen monoxide gas decomposes to form nitrogen gas and oxygen gas. How many grams of oxygen are formed when 10.0 g of dinitrogen monoxide decomposes? A) 0.275 g B) 3.64 g C) 7.27 g D) 14.5 g

B) 3.64 g

Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide: Pb2+(aq) + 2I-(aq) → PbI2(s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 0.700 mol of Pb(NO3)2(aq) to completely precipitate the lead? A) 2.54 × 10-3 mL B) 394 mL C) 197 mL D) 0.197 mL E) 0.394 mL

B) 394 mL

How many milliliters of a 0.266 M NaNO3 solution are required to make 150.0 mL of 0.075 M NaNO3 solution? A) 53.2 mL B) 42.3 mL C) 18.8 mL D) 23.6 mL E) 35.1 mL

B) 42.3 mL

What is the concentration of HCl in the final solution when 65 mL of a 12 M HCl solution is diluted with pure water to a total volume of 0.15 L? A) 2.8 × 10-2 M B) 5.2 M C) 28 M D) 5.2 × 103 M

B) 5.2 M

A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only phosphorus trichloride (PCl3). If it is the only product, what mass of PCl3 is formed? A) 30.15 g B) 54.93 g C) 140.01 g D) 79.71 g E) 91.86 g

B) 54.93 g

How many molecules of H2S are required to form 79.0 g of sulfur according to the following reaction? Assume excess SO2. 2 H2S(g) + SO2(g) → 3 S(s) + 2H2O(l) A) 1.48 × 1024 molecules H2S B) 9.89 × 1023 molecules H2S C) 5.06 × 1025 molecules H2S D) 3.17 × 1025 molecules H2S E) 2.44 × 1023 molecules H2S

B) 9.89 × 1023 molecules H2S

If the density of ethanol, C2H5OH, is 0.789 g/mL. How many milliliters of ethanol are needed to produce 15.0 g of CO2 according to the following chemical equation? C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) A) 6.19 mL B) 9.95 mL C) 19.9 mL D) 39.8 mL

B) 9.95 mL

What is the net ionic reaction for the following reaction in aqueous solutions: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) A) AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) B) Ag+(aq) + Cl-(aq) → AgCl(s) C) Ag+(aq) +NO3-(aq) +Na+(aq) + Cl- (aq) → Ag+(aq) +NO3-(aq) + Na+(aq) + Cl- (aq) D) Ag+(aq) +NO3-(aq) +Na+(aq) + Cl- (aq) → AgCl(s) +Na+(aq) + NO3-(aq)

B) Ag+(aq) + Cl-(aq) → AgCl(s)

Which of the following pairs of aqueous solutions will react to produce a precipitate? A) NH4NO3 + Li2CO3 B) Hg2(NO3)2 + LiI C) NaCl + Li3PO4 D) AgC2H3O2 + Cu(NO3)2 E) None of the above solution pairs will produce a precipitate.

B) Hg2(NO3)2 + LiI

When 280. mL of 1.50 × 10-4 M hydrochloric acid is added to 135 mL of 1.75 × 10-4 M Mg(OH)2, the resulting solution will be A) acidic. B) basic C) neutral. D) It is impossible to tell from the information given.

B) basic

What is the oxidation number of the chromium atom in Na2CrO4? A) -2 B) +2 C) +6 D) +7

C) +6

Determine the concentration of a solution prepared by diluting 25.0 mL of a stock 0.188 M Ca(NO3)2 solution to 150.0 mL. A) 1.13 M B) 0.0887 M C) 0.0313 M D) 0.0199 M E) 0.0501 M

C) 0.0313 M

Which of the following solutions will have the highest concentration of chloride ions? A) 0.10 M NaCl B) 0.10 M MgCl2 C) 0.10 M AlCl3 D) 0.05 M CaCl2 E) All of these solutions have the same concentration of chloride ions.

C) 0.10 M AlCl3

The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 M KOH solution. What is the concentration of the H3PO4 solution (in M)? A) 1.03 M B) 0.343 M C) 0.114 M D) 0.138 M E) 0.0461 M

C) 0.114 M

If the reaction of phosphate ion with water is ignored, what is the total concentration of ions in a solution prepared by dissolving 3.00 g of K3PO4 in enough water to make 350. mL of solution? A) 0.0101 M B) 0.0404 M C) 0.162 M D) 0.323 M

C) 0.162 M

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 M AgNO3 solution to completely precipitate the silver? 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

C) 0.535 g

What is the concentration of ions in a 0.25 M Al2(CO3)3 solution? A) 0.25 M B) 1.00 M C) 1.25 M D) 0.50 M E) 0.75 M

C) 1.25 M

What is the molar concentration of sodium ions in a 0.450 M Na3PO4 solution? A) 0.150 M B) 0.450 M C) 1.35 M D) 1.80 M

C) 1.35 M

How many moles of CuO can be produced from 0.900 mol of Cu2O in the following reaction? 2 Cu2O(s) + O2(g) → 4 CuO(s) A) 0.450 mol B) 0.900 mol C) 1.80 mol D) 3.60 mol

C) 1.80 mol

According to the following reaction, how many moles of Fe(OH)2 can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl2. FeCl2(aq) + 2 LiOH(aq) → Fe(OH)2(s) + 2 LiCl(aq) A) 3.97 × 10-2 moles B) 2.52 × 10-2 moles C) 1.99 × 10-2 moles D) 5.03 × 10-2 moles E) 6.49 × 10-2 moles

C) 1.99 × 10-2 moles

If the percent yield for the following reaction is 65.0%, how many grams of KClO3 are needed to produce 32.0 g of O2? 2 KClO3(s) → 2 KCl(s) + 3 O2(g) A) 53.1 g B) 81.7 g C) 126 g D) 283 g

C) 126 g

How many milliliters of a 9.0 M H2SO4 solution are needed to make 0.35 L of a 3.5 M solution? A) 0.14 mL B) 0.90 mL C) 140 mL D) 900 mL

C) 140 mL

How many of the following compounds are insoluble in water? KC2H3O2 CaSO4 SrS AlPO4 A) 0 B) 1 C) 2 D) 3 E) 4

C) 2

Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C8H18 with 4.00 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O A) 0.640 moles B) 64.0 moles C) 2.56 moles D) 16.0 moles

C) 2.56 moles

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H2O(l) → Ca(OH)2(s) A 4.50-g sample of CaO is reacted with 4.34 g of H2O. How many grams of water remain after the reaction is complete? A) 0.00 B) 0.00892 C) 2.90 D) 1.04 E) 0.161

C) 2.90

Based on the balanced chemical equation shown below, what volume of 0.250 M K2S2O3(aq), is needed to completely react with 24.88 mL of 0.125 M KI3(aq), according to the chemical equation: 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq). A) 6.22 mL B) 12.4 mL C) 24.9 mL D) 99.5 mL

C) 24.9 mL

Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 2NaN3(s) → 2Na(s) + 3N2(g) How many moles of N2 are produced by the decomposition of 2.88 mol of sodium azide? A) 1.92 B) 8.64 C) 4.32 D) 0.960 E) 1.44

C) 4.32

How many grams of oxygen are formed when 6.21 moles of KOH are formed? 4 KO(s) + 2 H2O(l) → 4 KOH(s) + O2(g) A) 19.9 g O2 B) 27.9 g O2 C) 49.7 g O2 D) 3.59 g O2 E) 11.7 g O2

C) 49.7 g O2

How many grams of H2 gas can be produced by the reaction of 54.0 grams of Al(s) with an excess of dilute hydrochloric acid in the reaction shown below? 2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g) A) 2.68 g B) 4.04 g C) 6.05 g D) 12.1 g

C) 6.05 g

How many milliliters of a 0.184 M NaNO3 solution contain 0.113 moles of NaNO3? A) 543 mL B) 163 mL C) 614 mL D) 885 mL E) 326 mL

C) 614 mL

What element is undergoing oxidation (if any) in the following reaction? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g) A) O B) H C) C D) both C and H E) None of the elements is undergoing oxidation.

C) C

The mixing of which pair of reactants will result in a precipitation reaction? A) CsI(aq) + NaOH(aq) B) HCl(aq) + Ca(OH)2(aq) C) K2SO4(aq) + Hg2(NO3)2(aq) D) NaNO3(aq) + NH4Cl(aq)

C) K2SO4(aq) + Hg2(NO3)2(aq)

Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N2O4 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol. N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) A) LR = N2H4, 59.0 g N2 formed B) LR = N2O4, 105 g N2 formed C) LR = N2O4, 45.7 g N2 formed D) LR = N2H4, 13.3 g N2 formed E) No LR, 45.0 g N2 formed

C) LR = N2O4, 45.7 g N2 formed

Which one of the following compounds is soluble in water? A) Cu3(PO4)2 B) CoS C) Pb(NO3)2 D) ZnCO3

C) Pb(NO3)2

Which of the following pairs of aqueous solutions will react to produce a precipitate? A) LiOH + Na2S B) (NH4)2SO4 + LiCl C) Sr(C2H3O2)2 + Na2SO4 D) KNO3 + NaOH E) None of the above solution pairs will produce a precipitate.

C) Sr(C2H3O2)2 + Na2SO4

When dissolved in water, KOH behaves as A) an acid that forms K+ and OH- ions. B) an acid that forms KO- and H+ ions. C) a base that forms K+ and OH- ions. D) a base that forms KO- and H+ ions.

C) a base that forms K+ and OH- ions.

HCl , HI , H2SO4, LiCl , and KI are all classified as A) acids. B) nonelectrolytes. C) strong electrolytes. D) weak electrolytes.

C) strong electrolytes.

HCl(aq) + (NH4)2S(aq) → H2S(g) + 2NH4Cl(aq) A) combustion B) acid base C) oxidation reduction D) gas evolution E) precipitation

D

A student dissolved 4.00 g of Co(NO3)2 in enough water to make 100. mL of stock solution. He took 4.00 mL of the stock solution and then diluted it with water to give 275. mL of a final solution. How many grams of NO3- ion are there in the final solution? A) 0.0197 g B) 0.0394 g C) 0.0542 g D) 0.108 g

D) 0.108 g

Determine the number of grams H2 formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 × 1023 atoms of Fe according to the following reaction. 2 HCl(aq) + Fe(s) → H2(g) + FeCl2(aq) A) 0.374 g B) 1.33 g C) 1.14 g D) 0.187 g E) 1.51 g

D) 0.187 g

What is the concentration of nitrate ions in a 0.125 M Mg(NO3)2 solution? A) 0.125 M B) 0.0625 M C) 0.375 M D) 0.250 M E) 0.160 M

D) 0.250 M

Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 10.00 mL of glacial acetic acid at 25°C in sufficient water to give 500.0 mL of solution. The density of glacial acetic acid at 25°C is 1.05 g/mL. A) 1.26 × 103 M B) 21.0 M C) 0.0210 M D) 0.350 M E) 3.50 × 10-4 M

D) 0.350 M

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. 4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g) A) 23.2 mol O2 B) 0.580 mol O2 C) 18.5 mol O2 D) 0.724 mol O2 E) 1.73 mol O2

D) 0.724 mol O2

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, HNO3 = 63.02 g/mol. 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) 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

D) 10.9 g H2O

How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 1.38 g of Fe2S3 if the percent yield for the reaction is 65.0%? 3 Na2S(aq) + 2 FeCl3(aq) → Fe2S3(s) + 6 NaCl(aq) A) 25.5 mL B) 43.1 mL C) 51.1 mL D) 102 mL

D) 102 mL

Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of MgSO3 and HI are mixed. A) 2 H+(aq) + SO32-(aq) → H2SO3(s) 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) → H2O(l) + SO2(g) E) No reaction occurs.

D) 2 H+(aq) + SO32-(aq) → H2O(l) + SO2(g)

Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of lithium sulfide and copper (II) nitrate are mixed. A) Li+(aq) + SO42-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + Li+(aq) + NO3-(aq) B) Li+(aq) + S-(aq) + Cu+(aq) + NO3-(aq) → CuS(s) + LiNO3(aq) C) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → Cu2+(aq) + S2-(aq) + 2 LiNO3(s) D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq) E) No reaction occurs.

D) 2 Li+(aq) + S2-(aq) + Cu2+(aq) + 2 NO3-(aq) → CuS(s) + 2 Li+(aq) + 2 NO3-(aq)

How many liters of a 0.0550 M KCl solution contain 0.163 moles of KCl? A) 3.37 L B) 1.48 L C) 8.97 L D) 2.96 L E) 1.12 L

D) 2.96 L

How many of the following compounds are soluble in water? Cu(OH)2 LiNO3 NH4Br K2S A) 0 B) 1 C) 2 D) 3 E) 4

D) 3

Based on the balanced chemical equation shown below, determine the mass percent of Fe3+ in a 0.7450 g sample of iron ore, if 22.40 mL of a 0.1000 M stannous chloride, SnCl2(aq), solution is required to completely react with the Fe3+ present in the ore sample. The chemical equation for the reaction is 2 Fe3+(aq) + Sn2+(aq) → 2 Fe2+(aq) + Sn4+(aq). A) 5.365% B) 8.396% C) 16.79% D) 33.58%

D) 33.58%

How many grams of NaCl are required to make 250.0 mL of a 3.000 M solution? A) 58.40 g B) 175.3 g C) 14.60 g D) 43.83 g

D) 43.83 g

What mass of N2 will be produced from the reaction of 50.0 g N2O4 with 45.0 g N2H4? N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g) A) 59.0 g B) 118 g C) 152 g D) 45.7 g

D) 45.7 g

Calculate the number of grams of solute in 500.0 mL of 0.189 M KOH. A) 148 B) 1.68 C) 5.30 × 103 D) 5.30 E) 1.68 × 10-3

D) 5.30

Lithium and nitrogen react in a combination reaction to produce lithium nitride: 6Li(s) + N2(g) → 2Li3N(s) In a particular experiment, 3.50 g samples of each reagent are reacted. The theoretical yield of lithium nitride is ________ g. A) 3.52 B) 2.93 C) 17.6 D) 5.85 E) 8.7

D) 5.85

According to the following reaction, what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution? 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq) A) 97.4 mL B) 116 mL C) 43.0 mL D) 86.1 mL E) 58.1 mL

D) 86.1 mL

Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: CaO(s) + H2O(l) → Ca(OH)2(s) In a particular experiment, a 5.00-g sample of CaO is reacted with excess water and 6.11 g of Ca(OH)2 is recovered. What is the percent yield in this experiment? A) 122 B) 1.22 C) 7.19 D) 92.5 E) 81.9

D) 92.5

Which of the following is not a strong electrolyte? A) CaS B) LiSO4 C) NH4OH D) CH3CH2CH3 E) Na2CO3

D) CH3CH2CH3

Which of the following compounds is an Arrhenius base? A) CH3OH B) CH3CO2H C) HOCl D) CsOH

D) CsOH

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and Fe(NO3)2 are mixed. A) K+(aq) + NO3-(aq) → KNO3(s) B) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → FeS(s) + 2 K+(aq) + 2 NO3-(aq) C) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 NO3-(aq) → Fe2+(aq) + S2-(aq) + 2 KNO3(s) D) Fe2+(aq) + S2-(aq) → FeS(s) E) No reaction occurs.

D) Fe2+(aq) + S2-(aq) → FeS(s)

Which of the following is an oxidation-reduction reaction? A) HCl(aq) + LiOH(aq) → LiCl(aq) + H2O(l) B) NaI(aq) + AgNO3(aq) → AgI(s) + NaNO3(aq) C) Pb(C2H3O2)2(aq) + 2 NaCl(aq) → PbCl2(s) + 2 NaC2H3O2(aq) D) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) E) All of the above are oxidation-reduction reactions.

D) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)

Which statement is correct for the following redox reaction? 5 Fe2+ + MnO4- +8H+ → 5 Fe3+ +Mn2+ + 4H2O A) Fe2+ is reduced. B) MnO4- is oxidized. C) Fe2+ is the oxidizing agent. D) MnO4- is the oxidizing agent.

D) MnO4- is the oxidizing agent.

Which of the following is a gas-evolution reaction? A) 2 C2H6(l) + 7 O2(g) → 4 CO2(g) + 6 H2O(g) B) 2 H2(g) + O2(g) → 2 H2O(g) C) LiCl(aq) + NaNO3(aq) → LiNO3(aq) + NaCl(g) D) NH4Cl(aq) + KOH(aq) → KCl(aq) + NH3(g) + H2O(l) E) None of the above are gas-evolution reactions.

D) NH4Cl(aq) + KOH(aq) → KCl(aq) + NH3(g) + H2O(l)

7.0 g of nitrogen is reacted with 5.0 g of hydrogen to produce ammonia according to the chemical equation shown below. Which one of the following statements is FALSE? N2(g) + 3 H2(g) → 2 NH3(g) A) 3.5 g of hydrogen are left over. B) Hydrogen is the excess reactant. C) Nitrogen is the limiting reactant. D) The theoretical yield of ammonia is 15 g.

D) The theoretical yield of ammonia is 15 g.

5.0 g of iron is reacted with 5.0 g of water according to the chemical equation shown below. Which one of the following statements is FALSE? 3 Fe(s) + 4 H2O(l) → Fe3O4(s) + 4 H2(g) A) 6.91 g of Fe3O4 are produced. B) 2.85 g of H2O are left over. C) Mass is conserved in this reaction. D) Water is the limiting reactant.

D) Water is the limiting reactant.

Consider the following balanced reaction. What mass (in g) of CO2 can be formed from 288 mg of O2? Assume that there is excess C3H7SH present. C3H7SH(l) + 6 O2(g) → 3 CO2(g) + SO2(g) + 4 H2O(g) A) 0.396 g CO2 B) 0.209 g CO2 C) 0.792 g CO2 D) 0.126 g CO2 E) 0.198 g CO2

E) 0.198 g CO2

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 in excess oxygen? A) 0.0317 B) 2.60 C) 0.770 D) 1.54 E) 0.385

E) 0.385

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

E) 17.22 g

Determine the theoretical yield of H2S (in moles) if 4.0 mol Al2S3 and 4.0 mol H2O are reacted according to the following balanced reaction. A possibly useful molar mass is Al2S3 = 150.17 g/mol. Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g) A) 12 mol H2S B) 4.0 mol H2S C) 18 mol H2S D) 6.0 mol H2S E) 2.0 mol H2S

E) 2.0 mol H2S

What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 solution? Hint: you will want to write a balanced reaction. A) 581 mL B) 173 mL C) 345 mL D) 139 mL E) 278 mL

E) 278 mL

How many milliliters of 0.132 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M NaOH? A) 0.521 B) 0.0120 C) 83.7 D) 0.0335 E) 29.9

E) 29.9

Determine the reducing agent in the following reaction. 2 Li(s) + Fe(C2H3O2)2(aq) → 2 LiC2H3O2(aq) + Fe(s) A) O B) H C) C D) Fe E) Li

E) Li

Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Al(C2H3O2)3 and LiNO3 are mixed. A) Al3+(aq) + 3 NO3-(aq) → Al(NO3)3(s) B) Li+(aq) + C2H3O2-(aq) → LiC2H3O2(s) C) Al3+(aq) + 3 NO3-(aq) + Li+(aq) + C2H3O2-(aq) → Al(NO3)3(aq) + LiC2H3O2(s) D) 3 Li+(aq) + (C2H3O2)33-(aq) → Li3(C2H3O2)3(s) E) No reaction occurs.

E) No reaction occurs.