Chemistry/Spring Final Review/Wohlers&Capps
a) Identify the limiting reactant for the reaction.
Cl2
c) dichlorine heptoxide
Cl2O7
a) Cl2O
Dichlorine monoxide
c) __HCl + __BaCl2 → ________________________ Type: ________________________
Doesn't Change (technically double replacement if you tried to do it)
b) Fe(C2H3O2)3
Fe - 23.97 %
a) FeCl2
Fe - 44 %
c) Fe(OH)2
Fe - 62.14 %
d) FeO
Fe - 77.72 %
h) BeH2
Linear; nonpolar
e) __Mg + __H2SO4 → _______________________ Type: ________________________
Mg + H2SO4 → single replacement
10. A compound is formed when 9.03 g Mg combines with 3.48 g N. What is the percent composition of this compound?
Mg - 72.2 % N - 27.8 %
b) (NH4)2C2O4
N - 22.6 % H - 6.45 % C - 19.35 % O - 51.6 %
a) dinitrogen monoxide
N2O
b) nitrogen dioxide
NO2
c) HNO3
Nitric acid (Nitrate)
f) NO
Nitrogen monoxide
b) NF3
Nitrogen triflouride
a) 94.1% O and 5.9% H MW = 34 g/mol
O2H2
a) 94.1% O, 5.9% H
OH
g) SF6
Octahedral; nonpolar
e) phosphorous pentabromide
PBr5
1. Write the formula for these compounds:
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11. Calculate the empirical formula of each compound: (% -> mass -> mole -> '/. by small -> x till whole)
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12. Determine the molecular formula for each compound.
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13. Write out balanced chemical formulas for the following reactions:
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14. Balance each equation and identify as to type:
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15. Complete the following equations and then balance and predict as to type:
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16. Write a balanced net ionic equation for the following reaction:
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17. Carbon disulfide is an important industrial solvent. It is prepared by the reaction of coke with sulfur dioxide: 5C + 2SO2 → CS2 + 4CO
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18. Methanol is used in the production of many chemicals. Methanol is made by reacting carbon monoxide and hydrogen at high temperature and pressure. CO + 2H2 → CH3OH
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19. According to the following equation: 2Al + 3Cl2 → 2AlCl3 Given 3.00 grams of aluminum and 5.3 grams of chlorine gas
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2. Name these compounds:
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22. Calculate the molarity of the following solution:
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3. Calculate the molar mass of each substance
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3. Name or give the formula of the following acids:
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4. Give the lewis dot structure shapes and tell whether or not they are polar or nonpolar:
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4. How many moles are in each of the following:
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5. How many grams are in each substance:
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6. How many Liters are in each of the following:
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7. Calculate the percent composition of each compound:
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CH 10
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CH 8
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Ch. 11
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Ch. 14
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Ch. 9
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c) CCl4
Tetrahedral; nonpolar
e) SO4 2-
Tetrahedral; nonpolar
a) PCl5
Trigonal bipyramidal; nonpolar
b) BF3
Trigonal planar; nonpolar
j) NO3 -1
Trigonal planar; nonpolar
f) PBr3
Trigonal pyramidal; polar
24.6 grams KCl in 750 mL solution
.44 molar
a) How many moles of CS2 are needed to form when 2.7 moles C reacts?
.54 mol of CS2
c) 5.3 x 10^22 molecules of F2
0.09 mol
a) 15.5 g of SiO2
0.258 mol
d) __C3H6O + __O2 → ________________________ Type: ________________________
1 C3H6O + 4 O2 → 3 CO2 + 3 H2O combustion
d) __Pb(NO3)2 + __NaI → __PbI2 + __NaNO3
1 Pb(NO3)2 + 2 NaI → 1 PbI2 + 2 NaNO3 double replacement
c) Calculate how many grams of the excess reactant remains after the reaction is complete.
1.66
b) 14.4 L CH4
10.3 g
c) CaCO3
100 g/mol
23. How many grams of the solute is needed to make 500 mL of a 2.0 M solution of KNO3
101 g
a) 1.50 mol of C5H12
108 g
b) How many moles of carbon are needed to react with 5.44 moles of SO2 ?
13.6 mol of C
d) (NH4)2SO4
132 g/mol
f) Br2
160 g/mol
a) 7.6 mol Ar
170
c) 3.21 x 10^24 molecules of H2O2
181 g
b) Calculate the number of grams of each reactant needed to produce 4.00 x 10^24 molecules of CH3OH.
186 g CO 26.6 g of H2
c) __C2H6 + __O2 → __CO2 + __H2O
2 C2H6 + 7 O2 → 4 CO2 + 3 H2O combustion
b) __Fe(OH)3 → _________________________ Type: ________________________
2 Fe(OH)3 → Fe2O3 + 3 H2O decomposition
a) sodium reacts with water to form hydrogen gas and sodium hydroxide
2 Na + 2 H2O → H2 + 2 NaOH
b) lead (IV) oxide decomposes to form lead (II) oxide and oxygen gas
2 PbO2 → 2 PbO + O2
25. How many mL of 0.500 M KCl solution would you need to dilute to make 100 mL of 0.100 M KCl?
20 mL
24. How many grams of NaCl is needed to make a 0.90% m/v solution if the solution volume is 2500 mL
22.5 g
c) How many grams of carbon monoxide form at the same time that 0.246 moles CS2 forms?
27.6 mol of CO
e) __Fe + __O2 → __Fe3O4
3 Fe + 2 O2 → 1 Fe3O4 synthesis
a) __Hf + __N2 → __Hf3N4
3 Hf + 2 N2 → 1 Hf3N4 synthesis
d) How many moles of SO2 are required to make 118 grams of CS2?
3.1 mol of SO2
b) 79.3 L of Cl2
3.54 mol
b) 44.4 g of C2H6
33.2
c) How many L of hydrogen gas are necessary to react with 2.85 grams of CO?
4.56 L of H2
a) How many grams of each reactant are needed to produce 360 grams of CH3OH?
45 g of H2 315 g og CO
b) Calculate the grams of the product formed.
6.6 g
20. According to the following equation: Sb2S3 + 3Fe → 2Sb + 3FeS When 15.0 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the percent yield of this reaction?
65.6 %
b) N2O3
76 g/mol
e) C4H9O2
89 g/mol
a) H3PO4
98 g/mol
AgNO3(aq) + AlCl3(aq) → ______________
AgCl(s) + Al(NO3)3(aq) Ag + Cl → AgCl
d) SO2
Bent; polar
c) 62.1% C, 13.8% H and 24.1% N
C3H8N
b) 50.7% C, 4.2% H and 45.1 % O MW = 142 g/mol
C6H6O4
f) carbon tetrachloride
CCl4
a) __Ca + __S → ________________________ Type: ________________________
Ca + S → CaS Synthesis
a) H2S
H - 5.87 % S - 94.13 %
f) sulfurous acid (Sulfite)
H2SO3
b) sulfuric acid (Sulfate)
H2SO4
c) hydrochloric acid reacts with calcium hydroxide to form calcium chloride and water
HCl + Ca(OH)2 → CaCl + H2O
d) chlorous acid (Chlorite)
HClO2
9. When a 14.2 g sample of mercury(II) oxide is decomposed into its elements by heating, 13.2 g Hg is obtained. What is the percent composition of the compound?
Hg - 93 % O - 7 %
b) 67.6% Hg, 10.8% S, and 21.6% O
HgSO4
a) HCl
Hydrochloric acid
e) H3PO4
Phosphoric acid (Phosphate)
e) SeO2
Selenium dioxide
d) trisilicon tetranitride
Si3N4
d) SiF4
Silicon tetraflouride
b) __Mg + __ H2SO4 → __MgSO4 + __H2
balanced single replacement
8. Which of these compounds have the highest percentage of iron?
d) FeO
21. Name and distinguish between the two components of a solution.
solute - what you mix (sugar) solvent - dissolves solute (water)
c) S4N4
tetrasulfur tetranitride
i) NH3
trigonal pyramidal; polar
