Honors Chemistry Chapter 11 Assessment

Identify the reactants and products in the chemical reaction: hydrogen gas and sodium hydroxide are formed when sodium is dropped into water
Reactants: sodium and water
Products: hydrogen and sodium hydroxide
Identify the reactants and products in the chemical reaction: in photosynthesis, carbon dioxide and water react to form oxygen gas and glucose
Reactants: cardon dioxide and water
Products: oxygen and glucose
Write sentences that completely describe each of the chemical reactions shown in this skeleton equation:
NH3(g) + O2(g) -(Pt)-> NO(g) + H2O(g)

Gaseous ammonia and oxygen react in the presence of a platinum catalyst to produce nitrogen monoxide gas and water vapor
Write sentences that completely describe each of the chemical reactions shown in this skeleton equation:
H2SO4(aq) + BaCl2(aq) –> BaSO4(s) + HCl(aq)

Aqeous solutions of sulfuric acid and barium chloride are mixed to produce a precipitate of barium sulfate and aqueous hydrochloric acid
Write sentences that completely describe each of the chemical reactions shown in this skeleton equation:
N2O3(g) + H2O(l) –>HNO2(aq)

The gas dinitrogen trioxide reacts with water to produce an aqeous solution of nitrous acid.
The equation for the formation of water from its elements, H2(g) + o2(g) –> H2O(l), can be “balanced” by changing the formula of the product to H2O2. Explain why this is correct.
A formula is a unique identifier of a substance. A different formula would indicate a different substance, not the one that is taking part in the reaction you are trying to balance.
Balance the following equation:
PbO2(s) –> PbO(s) + O2(g)

2PbO2(s) –> 2PbO(s) + O2(g)
Balance the following equation:
Fe(OH)3(s) –>Fe2O3(s) + H2O(s)

2Fe(OH)3(s) –>Fe2O3(s) + 3H2O(s)
Balance the following equation:
(NH4)2CO3(s)–>NH3(g) + H2O(g) + CO2(g)

(NH4)2CO3(s)–>2NH3(g) + H2O(g) + CO2(g)
Balance the following equation:
CaCl2(aq) + H2SO4(aq) + CaSO4(s) + HCl(aq)

CaCl2(aq) + H2SO4(aq) + CaSO4(s) + 2HCl(aq)
Write a balanced chemical equation for the following:
Mg(s) + O2(g) –>

2Mg(s) + O2(g) –> 2MgO(s)
Write a balanced chemical equation for the following:
P(s) + O2(g) –>diphosphorus pentoxide

4P(s) + 5O2(g) –>2P2O5(s)
Write a balanced chemical equation for the following:
Ca(s) + S(s) –>

Ca(s) + S(s) –> CaS(s)
Write a balanced chemical equation for the decomposition reaction:
Ag2O(s) –>

2Ag2O –> 4Ag + O2
Write a balanced chemical equation for the decomposition reaction:
ammonium nitrate –> dinitrogen monoxide + water

NH4NO3 –> N2O + 2H2O
Use the activity series of metals to write a balanced chemical equation for the following single-replacement reaction:
Au(s) + KNO3(aq) –>

no reaction
Use the activity series of metals to write a balanced chemical equation for the following single-replacement reaction:
Zn(s) + AgNO3(aq) –>

Zn(s) + 2AgNO3(aq) –> Zn(NO3)2(aq) + 2Ag(s)
Use the activity series of metals to write a balanced chemical equation for the following single-replacement reaction:
AL(s) + H2SO4(aq) –>

2AL(s) + 3H2SO4(aq) –> AL2(SO4)3(aq) + 3H2(g)
Write a balanced equation for the following double-replacement reaction:
H2C2O4(aq) + KOH(aq) –>

H2C2O4(aq) + 2KOH(aq) –> K2C2O4(aq) + 2H2O(l)
Write a balanced equation for the following double-replacement reaction:
CdBr2(aq) + Na2S(aq) –>
(Cadmium sulfide is a precipitate)

CdBr2(aq) + Na2S(aq) –> CdS(s) + 2NaBr(aq)
Write a balanced equation for the complete combustion of butene (C4H8)
C4H8(g) + 6O2(g) –> 4CO2(g) + 4h2O(g)
Write a balanced equation for the complete combustion of propanal (C3H6O)
C3H6O(l) + 4O2(g) –> 3CO2(g) + 3H2O(g)
Balance the equation and identify its type:
Hf(s) + N2(g) –>Hf3N4(s)

3Hf(s) + 2N2(g) –>Hf3N4(s)
combination
Balance the equation and identify its type:
Mg(s) + H2SO4(aq) –>MgSO4(aq) + H2(g)

Mg(s) + H2SO4(aq) –>MgSO4(aq) + H2(g)
single-replacement
Balance the equation and identify its type:
C2H6(g) + O2(g) –>CO2(g) + H2O(g)

2C2H6(g) + 7O2(g) –>4CO2(g) + 6H2O(g)
combustion
Balance the equation and identify its type:
Pb(NO3)2(aqA) + NaI(aq)–>PbI2(s) + NaNO3(aq)

Pb(NO3)2(aqA) + 2NaI(aq)–>PbI2(s) + 2NaNO3(aq)
double replacement
What is a distinguishing feature of every decomposition reaction?
a single reactant
What is a spectator ion?
an ion that does not participate in the reaction
Write a balanced net ionic equation for the following reaction:
HCl(aq) + Ca(OH)2(aq) –>

H+(aq) + OH-(aq) –>H2O(l)
Write a balanced net ionic equation for the following reaction:
AgNO3(aq) + AlCl3(aq) –>
(silver chloride is a precipitate)

Ag+(aq) + Cl-(aq) –>AgCl(s)
Complete the equation and then write a net ionic equation:
Al(s) + H2SO4(aq) –>

2Al(s) + 6H+(aq) –> 2AL3+(aq) + 3H2(g)
Complete the equation and then write a net ionic equation:
HCl(aq) + Ba(OH)2(aq)–>

H+(aq) + OH-(aq) –> H2O(l)
Complete the equation and then write a net ionic equation:
Au(s) + HCl(aq) –>

no reaction
Write a balanced chemical equation and use the necessary symbols from Table 11.1 to describe the reaction completely:
Bubbling chlorine gas through a solution of potassium iodide gives elemental iodine and a solution of potassium chloride

Cl2(g) + 2Kl(aq) –> I2(aq) + 2KCl(aq)
Write a balanced chemical equation and use the necessary symbols from Table 11.1 to describe the reaction completely:
Bubbles of hydrogen gas and aqueous iron (III) chloride are produced when metallic iron is dropped into hydrochloric acid

2Fe(s) + 6HCl(aq) –> 2FeCl3 (aq) + 3H2(g)
Write a balanced chemical equation and use the necessary symbols from Table 11.1 to describe the reaction completely:
Solid tetraphosphorus decaoxide reacts with water to produce phosphoric acide

P4O10(s) + 6H2O(l) –> 4H3PO4(aq)
The following equation is incorrect. Find the errors, then rewrite and balance the equation:
Cl2 + NaI –> NaCl2 + I

Cl2 + 2NaI –> 2NaCl + I2
The following equation is incorrect. Find the errors, then rewrite and balance the equation:
NH3 –> N + H3

2NH3 –> N2 + 3H2
The following equation is incorrect. Find the errors, then rewrite and balance the equation:
Na + O2 –> NaO2

4Na + O2 –> 2Na2O
Write balanced chemical equation for the double-replacement reactions that occur in aqueous solution:
Zinc sulfide is added to sulfuric acid

ZnS(aq) + H2SO4(aq) –> H2S(g) + ZnSO4(aq)
Write balanced chemical equation for the double-replacement reactions that occur in aqueous solution:
Sodium hydroxide reacts with nitric acid

NaOH(aq) + HNO3(aq) –> H2O(l) + NaNO3(aq)
Write balanced chemical equation for the double-replacement reactions that occur in aqueous solution:
solutions of potassium flouride and calcium nitrate are mixed

2KF(aq) + Ca(NO3)2(aq) –> CaF2(s) + 2KNO3(aq)
Write a balance chemical equation for the following combination reaction:
sodium oxide + water

Na2O(s) + H2O(l) –> 2NaOH(aq)
Write a balance chemical equation for the following combination reaction:
hydrogen + bromine

H2(g) + Br2(g) –> 2HClO4(aq)
Write a balance chemical equation for the following combination reaction:
dichlorine heptoxide + water

Cl2O7(l) + H2O(l) –> 2HClO4(aq)
Write a balanced chemical equation for the single-replacement reaction that takes place in aqueous solution. Write “no reaction” if a reaction does not occur:
Steel wool (iron) is placed in sulfuric acid

Fe(s) + H2SO4(aq) –> FeSO4(aq) + H2(g)
Write a balanced chemical equation for the single-replacement reaction that takes place in aqueous solution. Write “no reaction” if a reaction does not occur:
Mercury is poured into an aqeous solution of zinc nitrate

no reaction
Write a balanced chemical equation for the single-replacement reaction that takes place in aqueous solution. Write “no reaction” if a reaction does not occur:
Bromine reacts with aqueous barium iodide

Br2(l) + Bal2(aq) –> BaBr2(aq) + I2(aq)
Pieces of sodium and magnesium are dropped into separate water-filled test tubes (A and B). There is vigorous bubbling in Tube A but not in Tube B.
Which tube contains the sodium metal?

Tube A
Pieces of sodium and magnesium are dropped into separate water-filled test tubes (A and B). There is vigorous bubbling in Tube A but not in Tube B.
Write an equation for the reaction in the tube containing the sodium metal. What type of reaction is occurring in this tube?

2Na(s) + 2H2O(l) –> 2NaOH(aq) + H2(g)
single-replacement
Write a balanced equation for the complete combustion of the following compound (assume that the products are carbon dioxide and water):
octane (C8H18)

2C8H18 + 25O2 –> 16CO2 + 18H2O
Write a balanced equation for the complete combustion of the following compound (assume that the products are carbon dioxide and water):
glucose (C6H12O6)

C6H12O6 + 602 –> 6CO2 + 6H2O
Write a balanced equation for the complete combustion of the following compound (assume that the products are carbon dioxide and water):
ethanoic acid (HC2H3O2)

HC2H3O2 + 2O2 –> 2CO2 + 2H2O
Write a balanced chemical equation for the following decomposition reaction:
aluminum is obtained from aluminum oxide with the addition of a large amount of electrical energy

2Al2O3 -energy-> 4Al + 3O2
Write a balanced chemical equation for the following decomposition reaction:
Heating tin (IV) hydroxide gives tin (IV) oxide and water

SAn(OH)4 –delta symbol-> SnO2 + 2H2O
Write a balanced chemical equation for the following decomposition reaction:
Silver carbonate decomposes into silver oxide and carbon dioxide when it is heated

Ag2CO3 -delta symbol-> Ag2O + CO2
Write a balanced net ionic equation for the following reaction. The product that is not ionized is given:
H2C2O4 + KOH –> [H2O]

H+(aq) + OH-(aq) –> H2O(l)
Write a balanced net ionic equation for the following reaction. The product that is not ionized is given:
Na2S + HCl –> [H2S]

S2-(aq) + 2H+(aq) –> H2S(g)
Write a balanced net ionic equation for the following reaction. The product that is not ionized is given:
NaOH + Fe(NO3)3 –> [Fe(OH3)]

3OH-(aq) + Fe3+(aq) –> Fe(OH)3(s)
A yellow precipitate formed with aqueous solutions of sodium sulfide and cadmium nitrate were mixed in a beaker.
Write the formula of the yellow precipitate.

CdS(s)
A yellow precipitate formed with aqueous solutions of sodium sulfide and cadmium nitrate were mixed in a beaker.
Identify the spectator ions in the solution

Na+(aq)
NO3-(aq)
A yellow precipitate formed with aqueous solutions of sodium sulfide and cadmium nitrate were mixed in a beaker.
Write the net ionic equation for the reaction

Cd2+(aq) + S2-(aq) –> CdS(s)
Identify the type of reaction when aluminum reacts with bromine
combination
Identify the type of reaction when copper reacts with aqueous silver nitrate
single-replacement
Identify the type of reaction when propane (C3H8) reacts with oxygen
combustion
Identify the type of reaction when lead (II) nitrate reacts with potassium iodide
double-replacement
Write the equation when aluminum reacts with bromine
2Al(s) + 3Br2(l) –> 2ALBr3(s)
Write the equation when copper reacts with aqeous silver nitrate
CU(s) + 2AgNO3(aq) –> Cu(NO3)2(aq) + 2Ag(s)
Write the equation when propane (C3H8) reacts with oxygen
C3H8(g) + 5O2(g) –> 3CO2(g) + 4H2O(g)
Write the equation when lead (II) nitrate reacts with potassium iodide
Pb(NO3)2(aq) + 2Kl(aq) –> Pbl2(s) + 2KNO3(aq)
Write a balanced chemical equation when sodium iodide reacts with phosphoric acid
3Nal + H3PO4 –> 3HI + Na3PO4
What type of reaction occurs when sodium iodide reacts with phosphoric acid
double-replacement
Write a balanced chemical equation when potassium oxide reacts with water
K2O + H2O –> 2KOH
What type of reaction occurs when potassium oxide reacts with water
combination
Write a balanced chemical equation when heating sulfuric acid produces water, oxygen and sulfur dioxide
2H2SO4 -delta symbol-> 2H2O + O2 + 2SO2
What type of reaction occurs when heating sulfuric acid produces water, oxygen and sulfur dioxide
decomposition
Write a balanced chemical equation when aluminum reacts with sulfuric acid
2Al + 3H2SO4 –> 3H2 + Al2(SO4)3
What type of reaction occurs when aluminum reacts with sulfuric acid
single-replacement
Write a balanced chemical equation when pentane (C5H12) reacts with oxygen
C5H12 + 8O2 –> 5CO2 +6H2O
What type of reaction occurs when pentane (C5H12) reacts with oxygen
combustion
When pale yellow chlorine gas is bubbled through a clear, colorless solution of sodium iodide, the solution turns brown. What type of reaction is taking place?
single-replacement
When pale yellow chlorine gas is bubbled through a clear, colorless solution of sodium iodide, the solution turns brown. Write the net ionic equation
Cl2(g) + 2I-(aq) –> I2(aq) + 2Cl-(aq)
Fill in the missing reactant, and then balance the equation:
K(s) + _____________________ –> KOH(aq) + H2(g)

H2O(l)
2K(s) + 2H2O(l) –> 2KOH(aq) + H2(g)
Fill in the missing reactant, and then balance the equation:
C2H5OH(l) + ___________ –> CO2(g) + H20(g)

O2(g)
C2H5OH(l) + ___________ –> CO2(g) + H20(g)
Fill in the missing reactant, and then balance the equation:
Bi(NO3)3(aq) + __________________ –> Bi2S3(s) + HNO3(aq)

H2S(g)
2Bi(NO3)3(aq) + 3H2S(g) –> Bi2S3(s) + 6HNO3(aq)
Fill in the missing reactant, and then balance the equation:
Al(s) + _________________ –> AlBr3(s)

Br2(l)
2Al(s) + 3Br2(l) –> 2AlBr3(s)
Why is smoking not permitted near an oxygen source?
Because a fire will burn faster in an area of high oxygen concentration
What would happen if a match were struck in a room filled with oxygen?
It would burn more vigorously
Should sulfuric acid be stored next to sodium hydroxide? Explain your answer
No. NaOH is a base, and bases should not be stored next to acids because reactions between these two classes of chemicals generate heat
If sulfuric acid should not be stored next to sodium hydroxide, write a balanced chemical equation to support your answer.
H2SO4(aq) + 2NaOH(s) –> Na2SO4(aq) + 2H2O(l)