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TRANSCRIPT
AP Chemistry Summer
Prerequisite ReviewANSWER KEY
Visit us at chemistrywithrourke.weebly.com
Adapted from: Bergmann-Sams
DUE JULY 1PART A. COMPOUNDS AND EQUATIONSBalancing Ionic CompoundsGiven the names of the elements that form a compound, determine their ionic charge and write the chemical symbols for the compound.
EX: Lithium OxygenLi2O Li+ O2-
1. Sodium SulfurNa+ S2-
Na2S
2. Potassium ChlorineK+ Cl-
KCl
3. Rubidium SulfateRb+ SO4
2-
Rb2SO4
4. Magnesium NitriteMg2+ NO2
-
Mg(NO2)2
5. Strontium IodineSr2+ I-
SrI2
6. Aluminum PerchlorateAl3+ ClO4
-
Al(ClO4)3
7. Ammonium PhosphateNH4
+ PO43-
(NH4)PO4
8. Hydronium BromineH3O+ Br-
H3OBr
9. Cupric CarbonateCu2+ CO3
2-
CuCO3
10. Iron (II) IodateFe2+ IO3
-
Fe(IO3)2
11. Ferrous hydroxideFe2+ OH-
Fe(OH)2
12. Ferric NitrateFe3+ NO3
-
Fe(NO3)3
Given chemical symbols below, determine the ionic charges of each element and then write the balanced chemical symbol for each compound formed.
EX: Na ClO3 Na2CO3
1. H Pb2+
H2Pb
2. Li NO3
LiNO3
3. Be CO3
BeCO3
4. H SO3
H2SO3
5. Ca NCa3N2
6. Cs BrCsBr
7. Fe3+ FFeF3
8. Ag+ SeAg2Se
Naming Ionic CompoundsFor each ionic compound, list the cation(s), anion(s), chemical formula, and electron dot structure
1. sodium iodide Chemical Formula Electron Dot Structure
cations _____Na_______NaI
anions _____I________
2. magnesium chloride Chemical Formula Electron Dot Structure
cations ____Mg2+_______MgCl2
anions ____Cl-________
3. aluminum sulfide Chemical Formula Electron Dot Structure
cations ____Al3+________Al2S3
anions _____S2-______
4. iron (III) oxide Chemical Formula Electron Dot Structure
cations _____Fe3+_______Fe2O3
anions ______O2-______
5. stannous bromide Chemical Formula Electron Dot Structure
cations _____Sn2+_________SnBr2
anions _____Br-_______
6. plumbic oxide Chemical Formula Electron Dot Structure
cations ____Pb2+________ PbO
anions ____O2- ____Balance Chemical ReactionsRewrite each chemical equation with the correct coefficients necessary to balance the equation.
1. NaCO3(aq) + Ca(OH) (aq) _____ NaOH(aq) + _____ CaCO3(s)
Na2CO3(aq) + Ca(OH)2 (aq) ___2_ NaOH(aq) + _____ CaCO3(s)
2. KPO4(aq) + _____ MgCl(aq) _____ Mg(PO4) (s) + _____ KCl (aq)
2 K3PO4(aq) + ___3_ MgCl2(aq) _____ Mg3(PO4)2 (s) + ___6_ KCl (aq)
3. Cu (s) + ____ H2SO4 (aq) ____ CuSO4 (aq) + ____ H2O (l) + ____ SO2 (g)
Cu (s) + __2__ H2SO4 (aq) ____ CuSO4 (aq) + ___2_ H2O (l) + ____ SO2 (g)
4. FeS (s) + HCl (aq) FeCl (aq) + HS (g)
FeS (s) + 2 HCl (aq) FeCl2(aq) + H2S (g)
5. Fe (s) + CuNO3 (aq) Cu (s) + Fe(NO3) (aq)
Fe (s) + 2 CuNO3 (aq) 2 Cu (s) + Fe(NO3)2 (aq)
6. KI (aq) + Cl2 (g) KCl (aq) +I2 (aq)
2KI (aq) + Cl2 (g) 2 KCl (aq) + I2 (aq)
7. Al (s) + S (s) AlS (s)
2Al (s) + 3 S (s) Al2S3(s)
Reaction TypesThis is an instructional sheet to help you understand chemical reactions and to be able to predict the products of chemical reactions.There are 5 types of reactions in chemistry.
I. Combustiona. The combustion of an organic material
i. EX: C3H8 + 5O2 3CO2 + 4H2Oii. The products are always carbon dioxide and water. The only thing that changes is the
organic material and the coefficients needed to balance the equation.
II. Combinationa. A + B Xb. EX: 2Mg + O2 2MgO
III. Single-Replacementa. Use the Activity Series to determine if an elemental metal will replace the metal in a compound
based upon the reactivity of the metalsi. EX: Fe + 2AgNO3 Fe(NO3)2 + 2Ag
ii. EX: Cu + Zn(NO3)2 X or NRIV. Double-Replacement
a. The cations of two ionic compounds exchange anionic partnersi. EX: NaOH + HCl NaCl + HOH
V. Decompositiona. The opposite of a combination reactionb. A compound decomposes into elements and compoundsc. Typical products include CO2, H2, O2
i. EX: BaCO3 BaO + CO2
ii. 2Zn(OH)2 2ZnO + 2H2
iii. Ni(ClO4)2 NiCl2 + 8O2
d. There are tests for each type of product formed
Predict the products. Identify the reaction type. ALWAYS balance the equation.1. Zn2+ + Ca(OH)2 Ca + Zn(OH)2
Single replacement
2. LiCl + KBrO3 LiBrO3 + KClDouble replacement
3. 2C2H6 + 7O2 4CO2 + 6H2Ocombustion
4. 2 MgO + Δ 2 Mg + O2
decomposition
5. 2 Hydrogen + Oxygen 2H2Ocombination
Balance and Identify Chemical ReactionsBalance each equation with coefficients (all componds should already be balanced) and identify the reaction type.
1. 2Hf + 2N2 Hf2N4
combination
2. Mg + H2SO4 MgSO4 + H2
Single replacement
3. 2C2H6 + 7O2 4CO2 + 6H2O
combustion
4. Pb(NO3)2 + 2 NaI PbI2 + 2 NaNO3
Double replacement
5. 3Fe + 2O2 Fe3O4
combination
6. 2Pb(NO3)2 2PbO + 4NO2 + O2
decomposition
7. Hg(NO3)2 + 2NH4SCN Hg(SCN)2 + 2NH4NO3
Double replacement
8. (NH4)2SO4 + 2NaOH 2NH3 + 2H2O + Na2SO4
Decomposition or Double Replacement
Predict the products, balance, and identify the type of reaction
9. Al + H2SO4 H2 + Al2(SO4)3
Single replacement
10. 2HCl + Ba(OH)2 2H2O + BaCl2
Double replacement
11. 2Au + 2HCl 2AuCl + H2
Single Replacement
Decomposition and Synthesis ReactionsA synthesis reaction is the opposite of a decomposition reaction. This practice will help us recognize the products for common decomposition reactions1) Sodium + Oxygen
4Na + O2 2Na2O
2) Lithium + Sodium chloride
Li + NaCl LiCl + Na
3) Sodium chloride and heat
NaCl + heat Na + Cl2
4) Potassium chlorate
2KClO3 + heat 2KCl + 3O2
5) Copper (II) + Oxygen
2Cu + O2 2CuO
6) Aluminum + Hydrogen chloride
2Al + 6HCl 3H2 + 2AlCl3
7) Magnesium + Oxygen
2Mg + O2 2MgO
8) Silver + Chlorine
2Ag + Cl2 2AgCl
9) Aluminum oxide and heat
2Al2O3 + heat 4Al + 3O2
DUE AUGUST 1PART B. STOICHIOMETRYStoichiometry Worksheet: Molecule to Mass/Mole
1. How many molecules are there in 24 grams of FeF3?
1.28x1023 molecules FeF3
2. How many molecules are there in 450 grams of Na2SO4?
1.91x1024 molecules Na2SO4
3. How many grams are there in 2.3 x 1024 atoms of silver?
411.9 g Ag
4. How many grams are there in 7.4 x 1023 molecules of AgNO3?
208.8 g AgNO3
5. How many grams are there in 7.5 x 1023 molecules of H2SO4?
122.1 g H2SO4
6. How many molecules are there in 122 grams of Cu(NO3)2?
3.92x1023 molecules Cu(NO3)2
7. How many grams are there in 9.4 x 1025 molecules of H2?
312.3 g H2
8. How many molecules are there in 230 grams of CoCl2?
1.06x1024 CoCl2
Stoichiometry Worksheet: Moles and Moles1. Carbon disulfide is an important industrial solvent. It is prepared by the reaction of coke with sulfur
dioxide: 5C(s) + 2SO2(g) -----> CS2(s) + 4CO(g)
a. How many moles of CS2 form when 6.3 mol of C reacts? THIS EXAMPLE IS DONE FOR YOU!
6.3mol C 1 mol CS2 = 1.26 mol CS2
5 mol C2. How many moles of carbon are needed to react with 7.24 moles of SO2
18.1 mol C
3. Silver can be made according to the following equation:2AgNO3+ Ca Ca(NO3)2 + 2Ag
a. Balance the equationb. Identify the type of reaction Single Replacement
c. If 35.3 moles of silver nitrate are reacted how many moles of silver are produced?
35.3 mol Ag
4. How many moles of carbon dioxide are formed when 44-mol of CH4 is burned?
44 mol CO2
5. How many moles of calcium phosphate is formed when 32.5-mols of calcium nitrate reacts with sodium phosphate?
3Ca(NO3 )2+2Na3PO4→Ca3 (PO4 )2+6NaNO3
32 .5mol ?mol32 .5molCa(NO3 )2
1x
1molCa3 (PO4 )2
3molCa(NO3 )2=10 .8molCa3(PO4 )2
Stoichiometry Worksheet: Moles and Moles6. Car batteries are called lead storage batteries because of their use of large quantities of lead. These
batteries utilize the following equation.Pb + PbO2 +2H+ + 2HSO4
- 2PbSO4 + 2 H2O
34 . 3gPbO 2
1x
1molPbO2
239 gPbO2x
2molH 2O1molPbO2
x18gH 2O1molH 2O
=
5 .16 gH 2O34 . 3gPbO 2
1 x1molPbO2
239 gPbO2x
2molPbSO4
1molPbO2x
303gPbSO4
1molPbSO4=
¿87 . 0gPbSO 4
7. 32.5-g of ZnSO4 reacts to form how many grams of BaSO4 according to the following equation. a. Balance the equationb. Identify the type of reaction
32 .5 gZnSO4
1x
1molZnSO4
161gZnSO4x
1molBaSO4
1molZnSO4x
233gBaSO 4
1molBaSO4=
¿47 .0 gBaSO4
8. When sodium metal is added to water the resulting gas, Hydrogen can often explode. How many Liters of hydrogen gas is produced when 41.2-g of sodium is dropped into water. You must balance the equation in order to solve the problem.
Na + HOH NaOH + H2
41 .2gNa1
x1molNa23 gNa
x1molH 2
2molNax
22.4 LH2
1molH 2=
¿20 .1 LH 2
9. 43.5-grams of barium sulfate is formed from the reaction of barium nitrate and sodium sulfate. How many moles of sodium sulfate reacted?
Ba(NO 3 )2+Na2 SO4→BaSO 4+2 NaNO3
?mol 43 . 5g43 .5g BaSO4
1x
1molBaSO4
233gBaSO4x
1molNa2 SO4
1molBaSO4=0. 187molNa2 SO4
Stoichiometry Worksheet: Volume1. Barium oxide reacts with carbon dioxide to make Barium carbonate:
BaO + CO2 BaCO3
a. Balance the equationb. Identify the type of reaction Single Replacement
c. If 23.4 moles of barium oxide react, how many liters of CO2 are required at STP?
23 . 4molBaO1
x1molCO2
1molBaOx
22. 4 LCO2
1molCO2=524 LCO2
2. Ammonia, (NH3) is produced by reacting its elements with each other according to the following equation:
N2 + 3H2 2NH3
a. Balance the equationb. Identify the type of reaction Combination
c. If 34.3-L of nitrogen is reacted with hydrogen, how many liters at STP of ammonia will be formed?
34 . 3 LN2
1x
2LNH 3
molN 2=68 .6 LNH 3
3. Calculate the volume of carbon dioxide produced when 250 g of pentane, C5H12, burn. Assume the carbon dioxide is cooled to STP.
250 gC5H12
1x
1molC5H12
72 gC5H12x
5molCO2
1molC5H12x
22. 4 LCO2
1molCO2=
389 LCO2
4. Propane is a gas used often for backyard grills. How many Liters of CO2 is produced when 54.9-L of propane (C3H8) is burned according to the following equation. Again, you must balance the equation in order to solve the problem.
C3H8 + O2 CO2 + H2O
54 . 9 LC3H8
1x
3 LCO2
1molC3H8=165 LCO2
Stoichiometry Worksheet: Grams1. 14.5-g of cesium explosively reacts with water to form hydrogen and cesium hydroxide. How many
molecules of hydrogen were formed?
2Cs+2H 2O→2CsOH+H214 . 5g ?molec14 . 5gCs1
x1molCs133gCs
x1molH 2
2molCsx
6 . 02 x 1023molecH 2
1molH 2=
3 .28 x 1022molecH 2
2. How many molecules of chlorine are needed to react with 5.6 g of iron to form iron III chloride?
5 .6 gFe1
x 1molFe56gFe
x3molCl22molFe
x6 .02 x1023molecCl21molCl2
=
9 .03 x1022molecCl2
3. What mass of ammonia, NH3, is necessary to react with 2.1 x 1024 molecules of oxygen when ammonia (NH3) reacts with oxygen to form water and nitrogen dioxide?
2 .1 x1024molecO2
1x
1molO2
6 .02 x1023molecO2
x4molNH 3
7 molO2x
17 gNH 3
1molNH 3=
33 . 9gNH 3
4. 22.8-g of NaOH is reacted with hydrochloric acid. How many grams of water is formed?
NaOH+HCl→HOH+NaCl22 .8 g ?g22 .8gNaOH1
x1molNaOH40 gNaOH
x1molHOH1molNaOH
x 18gHOH1molHOH
=10 .3gHOH
5. 32.5-grams of iron III chloride reacts with silver nitrate. How many grams of silver chloride are formed?
3 .25 gCu(NO3)2
1x
1molCu(NO3 )2
187 . 5gCu(NO3 )2x
1molCu(OH )2
1molCu(NO3 )2x
97 .5 gCu(OH )2
1molCu(OH )2=
1 .69 gCu(OH )2
Stoichiometry Worksheet: Grams6. 34.5-grams of Lithium reacts with Chromium III chloride. How many grams of lithium chloride is
formed?
3 Li+CrCl3→3LiCl+Cr34 . 5g ?g34 . 5gLi1
x 1molLi7gLi
x3molLiCl3molLi
x42 . 5gLiCl1molLiCl
=209gLiCl
7. 43.5-grams of copper II sulfate is reacted with barium nitrate. How many grams of precipitate are formed?
8. Calculate the mass of silver needed to react with chlorine to produce 84 g of silver chloride.
CuSO4+Ba(NO3 )2→BaSO4( s )
+Cu(NO3 )2(aq)
43 .5g g?43 .5gCuSO4
1x
1molCuSO4
159. 5 gCuSO4x
1molBaSO4
1molCuSO4x
233gBaSO 4
1molBaSO4=
63 .5 gBaSO4
9. Silver nitrate reacts with sodium chloride to make the silver chloride and sodium nitrate. When 2.53 grams of silver nitrate is reacted. How many grams of silver chloride are formed?
2 .53 gAgNO3
1x
1molAgNO3
170 gAgNO3x1molAgCl
1molAgNO3x 143. 5gAgCl
1molAgCl=
2 .14 gAgCl
10. When 3.25 g of copper II nitrate reacts with ammonium hydroxide. How many grams of the precipitate will form?
3 .25 gCu(NO3 )2
1x
1molCu (NO3 )2
187 . 5gCu(NO3 )2x
1molCu (OH )2
1molCu (NO3 )2x
97 .5 gCu(OH )2
1molCu(OH )2=
1 .69 gCu(OH )2
Stoichiometry Worksheet: Limiting Reactants1. When 114.0 g of iron and 292.7 g of chlorine gas reacts, iron(III) chloride is formed.
2Fe+3Cl2→2FeCl3114g 292 .7g ?g114gFe1
x 1molFe56 gFe
x2molFeCl32molFe
x162 .5 gFeCl31molFeCl3
=331gFeCl
¿
¿ 3 ¿¿ ¿¿ ¿292 .7gCl2
1 x1molCl2
71 gCl2x
2molFeCl33molCl2
x162.5gFeCl3
1molFeCl3=447 gFeCl3 ¿ Fe is the LR because it yielded the smallest answer ¿
114gFe1 x 1molFe
56 gFe x3molCl22molFe x
71 gCl21molCl2
=217gCl2 usedup ¿292. 7−217g=75 .9gCl2 left ¿¿
2. 20 L of oxygen react with 1.0L of methyl alcohol, CH3OH.2CH 3OH+3O2→2CO2+4 H2O1 .0L 20L ?L1 .0 LCH 3OH1
x4 LH2O2 LCH 3OH
=2 LH 2O
20 LO2
1x
4 LH 2O3 LO2
=27 LH 2O
CH 3OH is the LR because it yielded the smallest answer1 .0 LCH 3OH1 x
3 LO2
2 LCH 3OH=1 .5 LO2
20 L−1 .5 L=18 . 5 LO2 Left
Stoichiometry Worksheet: Limiting Reactants3. 25 g of hydrazine, N2H4(l), and 66 g of hydrogen peroxide, H2O2(l), react to produce nitrogen gas and water.
N2 H 4+2H2O2→N2+4H2O25g 66g g? 25 gN2 H4
1x
1molN2H 4
32gN 2H4x
1molN 2
1molN 2H 4x
28gN 2
1molN 2=22 gN2
66 gH2O2
1x
1molH2O2
34 gH 2O2x
1molN 2
2molH 2O2x
28 gN 2
1molN 2=27 gN2
N2 H 4 is the LR because it yielded the smallest answer25 gN2 H4
1 x1molN2H 4
32gN 2H4x
2molH2O2
1molN 2H 4x
34 gH2O2
1molH 2O2=53 gH2O2
66 g−53g=13gH 2O2 leftover
4. 22.5 grams of lithium reacts with 33.5 grams of aqueous aluminum sulfate. This is a single replacement reaction.
6 Li+Al2( SO4 )3→3 Li2 SO 4+2 Al22 .5g 33 .5 g? 22 .5 gLi1
x 1molLi7g
x3molLi2 SO4
6molLix
110 gLi2 SO4
1molLi2 SO4=177gLi 2SO4
33 .5 gAl2 (SO4 )3
1x
1molAl2 (SO4 )3
342 gAl2 (SO4)3x
3molLi2 SO4
1molAl2 (SO4 )3x
110 gLi2 SO4
1molLi2 SO4=32gLi2 SO4
Al2 (SO4 )3 is the LR since it yields the smaller value33 .5 gAl2 (SO4 )3
1 x1molAl2 (SO4 )3
342 gAl2 (SO4)3x6molLi
1molAl2 (SO4 )3x7 gLi
1molLi =4 .1 gLi
22g−4 .1 g=18 gLiLeftover
Stoichiometry Worksheet: Percent Yield 1. 15.5-g of NH4Cl reacts with an excess of AgNO3. In the reaction 35.5-g AgCl is produced. NH4NO3 is the
other product. What is the percent yield?
15 .5 gNH 4Cl1
x1molNH 4Cl53 .5 gNH 4Cl
x1molAgCl1molNH 4Cl
x 143 .5 gAgCl1molAgCl
=
41 . 57gAgCl
%=35 .5g41.57 g
x100=85. 3 %
2. Potassium Chlorate decomposes according to the following reaction. 2KClO3 2KCl +3 O2
a. In an experiment 32.5-g of KClO3 is decomposed and 15.2-g of KCl is formed. What is the percent yield?
32 .5 gKClO3
1x
1molKClO 3
122. 5gKClO 3x2molKCl
2molKClO3x 74 .5gKCl
1molKCl=
¿19 .7 gKCl
%=15 .2g19 .7g
x 100=76 .9 %
3. Nitrogen gas reacts with hydrogen gas to make ammonia (NH3). 15.5-L of N2 reacts at STP to make 30-L of ammonia. What is the percent yield?
15 .5 LN 2
1x
2LNH 3
1 LN 2=31 LNH 3
%=30 L31 L
x100=97 %
4 What is the percent yield of oxygen gas if 54L of O2 can be obtained from the thermal decomposition of 500.0 g of potassium chlorate?
KClO3 KCl + O2
2 KClO3→2 KCl+3O2500 . 0g 54L500 gKClO3
1x
1molKClO3
122 .5 gKClO3x
3molO2
2molKClO3x
22. 4 LO 2
1molO 2=137 LO2
%=54 L137 L
x100=39. 4%
Stoichiometry Worksheet: Mixed Problems1. How many grams of water are formed when 12.5-g of hydrogen reacts with oxygen?
12 .5 gH2
1x
1molH 2
2gH 2x
2molH 2O2molH 2
x18gH 2O1molH 2O
=
¿112.5 gH 2O
2. How many liters of carbon dioxide are formed when 12.3-g of sodium carbonate reacts with 2.0-L of hydrogen chloride. The reaction is printed below:
Na2CO3 + HCl NaCl + H2O + CO2
12 .3 gNa2CO 3
1x
1molNa2CO 3
106 Na2CO3x
1molCO2
1molNa2CO3x
22 . 4 LCO2
1molCO2=
¿2 .60 LCO2
2 .0 LHCl1 x
1 LCO2
2 LHCl =1 .0 LCO2
¿1 .0 LCO2 : Answer because it is the lowest
3. How many grams of precipitate are formed when 24.3-g of zinc nitrate reacts with 20.5-g of sodium phosphate?
24 .3gZn(NO3 )2
1x
1molZn(NO 3 )2189gZn(NO3 )2
x1molZn3 (PO 4 )2
3molZn(NO3)2x
385 gZn3(PO 4 )2
1molZn3 (PO4 )2=
¿16 .5 gZn3(PO4 )2 :: This is the answer b/c it is lowest20 .5 gNa3PO 4
1x
1molNa3PO4
164 gNa3PO4x
2molNa3PO4
3molZn(NO 3 )2x
385 gZn3 (PO4 )2
1molZn3(PO4 )2=
¿32 .1gZn3 (PO 4 )2
4. How many liters of oxygen are produced when 3.25-g of KClO3 decomposes into KCl and O2?
3 .25 gKClO3
1x
1molKClO3
122.5 gKClO3x
3 molO2
2molKClO3x
22 .4 LO2
1molO2=
¿0 . 89LO2