Mr. Rivas
The Mole WS
SET 1
01.
How many moles of Na are in 42 g of Na?
02.
How many moles of O are in 8.25 g of O?
03.
How much does 2.18 mol of Cu weigh?
04.
What is the mass of 0.28 mol of iron?
05.
How many atoms are in 7.2 mol of chlorine?
06.
How many atoms are in 36 g of bromine?
07.
How many moles are in 1.0 x 109 atoms?
08.
What is the mass of 1.20 x 1025 atoms of sulfur?
09.
How many moles of CO molecules are in 52 g of CO?
10.
How many moles of C2H6 are in 124 g?
11.
How many moles of CCl4 are there in 56 g?
12.
How much does 2.50 mol of H2SO4 weigh?
13.
How much does 0.25 mol of Fe2O3 weigh?
14.
How many molecules are there in 52 g of CO?
15.
How many formula units are in 22.4 g SnO2?
16.
How many molecules are in 116 g CCl4?
17.
What is the mass of 3.01 x 1023 formula units of Fe2O3?
18.
What is the mass of 1.2 x 1025 molecules of CO?
19.
How many O atoms are in 1.25 mol of SO2?
20.
How many moles of O atoms do you have when you have 1.20 x 10 25 N2O5 molecules?
21.
How many formula units are in 5.33 mol of CuCl2?
22.
How many copper atoms are in 5.33 mol of CuCl2?
23.
How many moles of Cl atoms are in 5.33 mol of CuCl2?
24.
How many moles of CuCl2 contain 1.2 x 1023 atoms of Cl?
25.
How many O atoms are in 3.15 mol of SnO2?
26.
How many H atoms are in 17.5 g (NH4)2C2O4?
Answers
01) 1.8 mol Na
02) 0.516 mol O
03) 139 g Cu
04) 16 g Fe
05) 4.3 x 1024 Cl atoms
06) 2.7 x 1023 Br atoms 07) 1.7 x 10-15 mol 08) 639 g S 09) 1.9 mol
10) 4.12 mol
11) 0.36 mol
12) 245 g 13) 40.g 14) 1.1x1024 molecules
15) 8.95x1022 formula units
23
2
16) 4.54x10 molecules 17) 79.9 g Fe2O3 18) 5.6x10 g CO 19) 1.51 x 1024 O atoms
20) 99.7 mol O 21) 3.21x1024 formula units 22) 3.21 x 1024 Cu atoms 23) 10.7 mol of Cl atoms
24) 0.10 mol CuCl2 25) 3.79x1024 O atoms 26) 6.79x1023 H atoms
SET 2
01. The number of atoms in 1.0 mole of argon.
02. The number of atoms in 3.0 moles of helium.
03 The number of molecules in 1.0 mole of oxygen gas.
04. The number of molecules in 1.0 mole of water.
05. The number of atoms in 1.0 mole of water.
06. The number of oxygen atoms in 1.0 mole of water.
07. The number of hydrogen atoms 1.0 mole of water
08. The number of molecules in 1.0 mole of sodium carbonate (Na2CO3), washing soda.
09. The number of molecules in 0.25 mole of sodium carbonate.
10. The number of oxygen atoms in 1.0 mole of sodium carbonate.
11. The number of oxygen atoms in 0.25 mole of sodium carbonate.
12. The mass of 1.0 mole of sodium carbonate.
13. The mass of oxygen in 1.0 mole of sodium carbonate.
14. The number of moles in 212.0 grams of sodium carbonate.
15. The number of grams in 0.75 mole of water.
16. The number of moles of water in 1.800 grams of water.
17. The number of atoms in 12 grams of carbon.
18. The number of atoms in 3.0 grams of carbon.
19. The number of atoms in 600.0 grams of carbon.
20. The mass of 1.80 x 1024 atoms of carbon.
21. The mass of 3.01 x 1023 molecules of water.
22. The number of atoms in 3.01 x1023 molecules of water.
23. The number of molecules in 36.0 grams of water.
24. The number of atoms in 36.0 grams of water.
25. The number of hydrogen atoms in 36.0 grams of water.
26. The number of atoms in 4.4 x1022 grams of carbon dioxide.
27. The number of moles in 3.7 x10-6 grams of carbon dioxide.
28. The number of moles of atoms found in 1.00 x103 grams of calcium carbonate, CaCO3.
29. The number of molecules in 7.100 grams of chlorine gas (be careful with chlorine gas).
30.The number of moles of chlorine atoms in 7.100 grams of chlorine gas.
Answers
01) 6.0E23
07) 1.2E24
13) 48
19) 3.0E25
25) 2.40E24
02) 1.8E24
08) 6.0E23
14) 2.000
20) 36.0
26) 1.8 E45
03) 6.0E23
09) 1.5E23
15) 14
21) 9.00
27) 8.4E-8
04) 6.0E23
10) 1.8E24
16) 0.1000
22) 9.03E23
28) 5.00 E1
05) 1.8E24
11) 4.5E23
17) 6.0E23
23) 1.20E24
29) 6.028 E22
06) 6.0E23
12) 106
18) 1.5E23
24) 3.60E24
30) 2.003 E-1
Mr. Rivas
Predicting Products of Chemical Reactions WS
This worksheet is designed to help you predict products of simple reactions of the four basic reaction types
(synthesis, decomposition, single replacement, and double replacement) and combustion reactions.
For the first few reactions, the type of reaction is listed, you should predict the products, then balance them. Further questions
just have the reactants listed and you should decide on the type of reaction, as well as the correct products. Many of these
reactions fall into the category of redox reactions, though do not let that confuse you...each can be described in terms of the
four basic reaction types (except the combustion reactions).
a. Combustion:
C6H12
+
O2

b. Combustion:
C4H6
+
O2

c. Combustion:
C6H10O3
+
O2
+
I2

2. Double displacement:
CuCl2
+
H2S
3. Double displacement:
NaOH +
1. Synthesis:
Mg


HClO4 
4. Decomposition:
ZnCO3 +
heat

5. Single replacement:
HCl
+
Zn

6. ________________
Na
+
MgCl2 
7. ________________
CaCl2
+
K2CO3 
8. ________________
K
+
Cl2
9. ________________
BaCl2
+
K3PO4 

10. ________________
H2SO4 +
KOH

11. ________________
Al2(CO3)3
+
heat
12. ________________
Al
O2

13. ________________
Pb(NO3)2
+
KOH
14. ________________
H2SO4 +
BaCl2

15. ________________
Ca
AgCl

16. ________________
H3PO4 +
FeBr3

17. ________________
Li
+
N2

18. ________________
HCl
+
Mg(OH)2

19. ________________
Mg(OH)2
+
heat

20. ________________
Fe(OH)3
+
heat
+
+



Balance the following reaction equations and classify each as to type of chemical reaction. For word
equations, write out the formulas before balancing.
21. Na2O + P4O10 → Na3PO4
22. C12H22O11 + O2 → CO2 + H2O
23. MnO2 + Al → Al2O3 + Mn
24. barium nitrate + sulfuric acid → barium sulfate + nitric acid
25. aluminum sulfate + sodium hydroxide → aluminum hydroxide + sodium sulfate
Complete and balance each of the following reactions.
26. Al + SnCl2 →
27. Ca + H2O →
28. Cl2 + NaBr →
29. Pb + HCl →
30. Zn + KCl →
31. Pb(NO3)2 + K2CrO4 →
32. ZnCO3 + H3PO4 →
33. Ca(OH)2 + HC2H3O2 →
34. FeCl3 + NaOH →
35. FeSO4 + (NH4)2S →
Convert each of the word equations into a balanced chemical equation.
36. magnesium + oxygen 
37. mercuric oxide (+heat) 
38. carbon + oxygen 
39. carbon + oxygen 
40. hydrogen + oxygen 
41. water (+electric current) 
42. methane + oxygen 
43. aluminum + oxygen 
44. sodium + oxygen 
45. sodium oxide + water 
46. sodium + water 
47. sulfur + oxygen 
48. sulfur + oxygen (+ catalyst) 
49. sulfur trioxide + water 
50. nitrogen + hydrogen 
51. hydrogen + chlorine 
52. ammonia + hydrogen chloride 
53. ammonium chloride + silver nitrate 
54. zinc + sulfuric acid 
55. zinc + sulfur 
56. zinc sulfide + sulfuric acid 
57. hydrogen sulfide + sulfur dioxide 
oride
Mr. Rivas
Chemical Reactions
Write balanced equations for the following word equations.
1. potassium chloride + silver nitrate  potassium nitrate + silver chloride
2. aluminum hydroxide + sodium nitrate  aluminum nitrate + sodium hydroxide
3. iron metal + copper(II) sulfate iron(II) sulfate + copper metal
4. aluminum metal + copper(II) chloride  aluminum chloride + copper metal
5. potassium bromide  potassium metal + bromine
6. calcium carbonate  calcium oxide + carbon dioxide gas
7. zinc metal + oxygen gas --> zinc oxide
8. chlorine gas + sodium metal  sodium chloride
9. aluminum sulfate + barium chloride  aluminum chloride + barium sulfate
10. beryllium fluoride + magnesium  magnesium fluoride + beryllium
11. sodium hydrogen carbonate  sodium carbonate + carbon dioxide + water
Complete the word equation for the following chemical equations and indicate the type of reaction: S =
synthesis, D = Decomposition, SR = Single replacement, DR = Double replacement, C = Combustion.
____ 12. aluminum sulfate + calcium phosphate  ______________________________
____ 13. magnesium chloride + silver nitrate  ________________________________
____ 14. sodium chlorate  ______________________________________________
____ 15. hydrogen gas + oxygen gas  _______________________________________
____ 16. zinc metal + copper(II) nitrate  ____________________
____ 17. sulfurous acid (H2SO3)  water + sulfur dioxide
____ 18. copper(II) oxide + sulfuric acid. H2SO4  _______________________________
____ 19. nitrogen gas + hydrogen gas  ammonia (NH3)
____ 20. sodium iodide + chlorine gas  _____________________________________
____ 21. copper(II) hydroxide  copper(II) oxide + water
____ 22. ammonia gas (NH3) + hydrochloric acid (HCl)  (hint: single product) ___________
____ 23. potassium metal + water (hint: H+OH-)  ______________________________
____ 24. propane (C3H8) + oxygen  (hint: two products) __________________________
Balance the following chemical reactions and indicate the type of reaction:
1. H2 + O2  H2O
2. S8 + O2  SO2
3. HgO  Hg + O2
4. Zn + HCl  ZnCl2 + H2
5. Na + H2O  NaOH + H2
6. C10H16 + Cl2  C + HCl
7. Si2H2 + O2  SiO2 + H2O
8. Fe + O2  Fe2O3
9. C7H6O2 + O2  CO2 + H2O
10. FeS2 + O2  Fe2O3 + SO2
11. Fe2O3 + H2  Fe + H2O
12. K + Br2  KBr
13. C2H2 + O2  CO2 + H2O
14. H2O2  H2O + O2
15. C7H16 + O2  CO2 + H2O
16. SiO2 + HF  SiF4 + H2O
17. KClO3  KCl + O2
18. KClO3  KClO4 + KCl
19. P4O10 + H2O  H3PO4
20. Sb + O2  Sb4O6
21. C2H8 + O2  CO2 + H2O
22. Fe2O3 + CO  Fe + CO2
23. PCl5 + H2O  HCl + H3PO4
24. H2S + Cl2  S8 + HCl
25. Fe + H2O  Fe2O3 + H2
26. N2 + H2  NH3
27. N2 + O2  N2O
28. CO2 + H2O  C6H12O6 + O2
29. SiCl4 + H2O  H4SiO4 + HCl
30. H3PO4  H4P2O7 + H2O
31. CO2 + NH3  OC(NH2)2 + H2O
32. Al(OH)3 + H2SO4  Al2(SO4)3 + H2O
33. Fe2(SO4)3 + KOH  K2SO4 + Fe(OH)3
34. H2SO4 + HI  H2S + I2 + H2O
35. Al + FeO  Al2O3 + Fe
36. Na2CO3 + HCl  NaCl + H2O + CO2
37. P4 + O2  P2O5
38. K2O + H2O  KOH
39. Al + O2  Al2O3
40. Na2O2 + H2O  NaOH + O2
41. C + H2O  CO + H2
42. H3AsO4  As2O5 + H2O
43. Al2(SO4)3 + Ca(OH)2  Al(OH)3 + CaSO4
44. FeCl2 + NH4OH  Fe(OH)2 + NH4Cl
45. Ca3(PO4)2 + SiO2  P4O10 + CaSiO3
46. N2O5 + H2O  HNO3
47. Al + HCl  AlCl3 + H2
48. H3BO2  H4B6O11 + H2O
49. Mg + N2  Mg2N2
50. NaOH + Cl2  NaCl + NaClO + H2O
Mr. Rivas
Empirical Formulas WS
01. A substance is 36.1% by weight calcium and 63.9% chlorine.
a) In 100.g of this substance, how many grams of Ca would there be?
b) In a 100.g of this substance, how many grams of Cl would there be?
c) How many moles of Ca are there?
d) How many moles of Cl are there?
e) What is the ratio, moles of Ca to moles of Cl?
f.) How many Cl’s are there for each Ca?
g) What is the empirical formula of this compound?
02. A compound is 43.4%Na, 11.3%C, 45.3%O.
a) In a 100.g sample of this substance there will be: (fill-in setup/solve)
_____ g Na and ____ mol Na
_____ gC = and ____ mol C
_____ gO = and ____ mol O
b) What is the ratio of mol Na to mol C?
c) What is the ratio of mol C to mol O?
d) What is the empirical formula for this compound?
03. A compound is 2.46%H, 39.1%S, 58.5%O. What is its empirical formula?
04. Calomel is the common name of a white powder once used in the treatment of syphilis. Its
composition is 84.98% mercury and 15.02% chlorine. What is its empirical formula?
05. A sample of an unknown compound with a mass of 2.571 grams was found to contain 1.102
grams of C and 1.469 grams of oxygen. What is its empirical formula?
06. When a sample with a mass of 2.448 grams of compound present in liquified petroleum gas
was analyzed, it was found to contain 2.003 grams of carbon and 0.4448 grams of
hydrogen. What is its empirical formula?
07 Barium carbonate, a white powder used in paints, enamels, and ceramics, has the following
composition: Ba, 69.58%; C, 6.090%; O, 24.32%. What is its empirical formula?
08. Realgar (re-Al-gar) is a deep red pigment used in painting. A 0.6817 grams sample was found
to contain 0.4774 grams of arsenic; the remainder was sulfur. What are the empirical
formula
09. The molecular formula of the antifreeze ethylene glycol is C 2H6O2. What is the empirical
formula? Ans: CH3O
10. A well-known reagent in analytical chemistry, dimethylglyoxime, has the empirical formula
C2H4NO. If its molar mass is 116.1 g/mol, what is the molecular formula of the compound?
Ans: C4H8N2O2.
11. Nitrogen and oxygen form an extensive series of oxides with the general formula NxOy. One
of them is a blue solid that comes apart, reversibly, in the gas phase. It contains 36.84% N.
What is the empirical formula of this oxide? Ans: N2O3
12. A sample of indium chloride weighing 0.5000 g is found to contain 0.2404 g of chlorine. What
is the empirical formula of the indium compound? Ans: InCl3
13. What is the empirical formula of a substance composed 56.6% potassium, 8.68% carbon, and
34.7% oxygen.
14. What is the empirical formula of a compound composed of 3.26 gof arsenic and 1.04 g of
oxygen?
15. An unknown compound is analyzed and found to consist of 24.3 % carbon, 4.1% hydrogen,
and 71.6 % chlorine. If the molecular mass of the compound is 98.8, what is the molecular
formula of the compound?
16. What is the empirical formula of a substance composed 49.89% strontium, 13,67% carbon,
and 36.44% oxygen?
17. An unknown compound is analyzed and found to consist of 49.0 % carbon, 2.7 % hydrogen,
and 48.2 % chlorine. If the molecular mass of the compound is 150, what is the molecular
formula of the compound?
18. Find the molecular formula for a compound with percentage composition 85.6 % C, 14.4 % H,
and molecular mass 42.1.
19 What is the molecular formula of a substance with empirical formula TlC2H2O3 and molecular
mass 557?
20. Hydroquinone is an organic compound commonly used as a photographic developer. It has a
molecular weight of 110 g/mole and a composition of 65.45% C, 5.45 % H, and 29.09 % O.
Calculate the molecular formula of hydroquinone.
21. In a previous problem, the empirical formula of a compound of phosphorus and oxygen was
found to be P2O5. Experimentation shows that the molar mass of this compound is 283.89g.
What is the compounds molecular formula.
22. The empirical formula for trichloroisocyanuric acid, the active ingredient in many household
bleaches, is OCNCl. The molar mass of this compound is 232.41g. What is the molecular
formula of trichloroisocyanuric acid.
23. The molar mass of a compound is 92g. Analysis of a sample of the compound indicates that it
contains 0.606g N and 1.390g O. Find its molecular formula.
24. Determine the molecular formula of a compound with an empirical formula of NH2 and a
formula mass of 32.06 amu.
25. A compound that combines in a fixed amount with one or more molecules of water is known as a hydrate. In
lab, a 5.00-g sample of hydrated barium chloride, BaCl2•xH2O, is heated to drive off the water. After heating,
4.26 g of anhydrous barium chloride, BaCl2, remains. What is the value of x in the hydrate’s formula?
26. The oxygen-carrying protein known as hemoglobin is 0.335% Fe by mass and contains exactly four Fe atoms
per hemoglobin molecule. Calculate the protein’s molar mass.
27. Halothane is an anesthetic that is 12.17% C, 0.51% H, 40.48% Br, 17.96% Cl and 28.87% F by mass. What is
the compound’s molar mass if each molecule contains exactly one hydrogen atom?
28. A compound that is 31.9% K and 28.9% Cl by mass decomposes when heated to give O2 and a compound that
is 52.4% K and 47.6% Cl by mass. Write a balanced chemical equation for this reaction.
Mr. Rivas
Stoichiometry WS-01
01. Na2SiO3 (s) + 8 HF(aq)  H2SiF6 (aq) + 2 NaF(aq) + 3 H2O (l)
a. How many moles of HF are needed to react with 0.300 mol of Na2SiO3?
b. How many grams of NaF form when 0.500 mol of HF reacts with excess Na 2SiO3?
c. How many grams of Na2SiO3 can react with 0.800 g of HF?
02. C6H12O6 (aq)  2 C2H5OH (aq) + 2 CO2 (g)
a. How many moles of CO2 are produced when 0.400 mol of C6H12O6 reacts in this fashion?
b. How many grams of C6H12O6 are needed to form 7.50 g of C2H5OH?
c. How many grams of CO2 form when 7.50 g of C2H5OH are produced?
03. Fe2O3 (s) + CO (g)  Fe(s) + CO2 (g) (unbalanced!)
a. Calculate the number of grams of CO that can react with 0.150 kg of Fe 2O3
b. Calculate the mass of Fe and the mass of CO2 formed when 0.150 kg of Fe2O3 reacts
04. 2 NaOH (s) + CO2 (g)  Na2CO3 (s) + H2O (l)
a. Identify the limiting reactant when 1.85 mol NaOH and 1.00 mol CO 2 are allowed to react?
b. How many moles of Na2CO3 can be produced?
05. C6H6 + Br2  C6H5Br + HBr
a. What is the theoretical yield of C6H5Br when 30.0 g of C6H6 reacts with 65.0 g or Br2?
b. If the actual yield of C6H5Br was 56.7 g, what is the percent yield?
06. Silver sulfide (Ag2S) is the common tarnish on silver objects. What weight of silver sulfide can
be made from 1.23 mg of hydrogen sulfide (H2S) obtained from a rotten egg? The reaction of
formation of silver sulfide is given below:
Ag(s) + H2S(g) + O2(g)  Ag2S(s) + H2O(l)
(Equation must first be balanced.)
07 A somewhat antiquated method for preparing chlorine gas involves heating hydrochloric acid
with pyrolusite (manganese dioxide), a common manganese ore. (Reaction given below.) How
many kg of HCl react with 5.69 kg of manganese dioxide?
HCl(aq) + MnO2(s)  H2O(l) + MnCl2 (aq) + Cl2(g) (Equation must first be balanced.)
08. Given the following equation: 2 C4H10 + 13 O2  8 CO2 + 10 H2O, show what the following
molar ratios should be.
a. C4H10 / O2
b. O2 / CO2
c. O2 / H2O
d. C4H10 / CO2 e. C4H10 / H2O
09. Given the following equation: 2 KClO3  2 KCl + 3 O2
How many moles of O2 can be produced by letting 12.00 moles of KClO3 react?
10. Given the following equation: 2 K + Cl2  2 KCl
How many grams of KCl is produced from 2.50 g of K and excess Cl2. From 1.00 g of Cl2 and
excess K?
11. Given the following equation: Na2O + H2O  2 NaOH
a) How many grams of NaOH is produced from 1.20 x 102 grams of Na2O?
b) How many grams of Na2O are required to produce 1.60 x 102 grams of NaOH?
12. Given the following equation: 8 Fe + S8  8 FeS
a) What mass of iron is needed to react with 16.0 grams of sulfur?
b) How many grams of FeS are produced?
13. Given the following equation: 2 NaClO3  2 NaCl + 3 O2
a) How many grams of O2 will be produced from 12.00 moles of NaClO3?
b) How many grams of NaCl are produced when 80.0 grams of O2 are produced?
14. Given the following equation: Cu + 2 AgNO3  Cu(NO3)2 + 2 Ag
a) How many moles of Cu are needed to react with 3.50 moles of AgNO3?
b) If 89.5 grams of Ag were produced, how many grams of Cu reacted?
15. Molten iron and carbon monoxide are produced in a blast furnace by the reaction of iron(III)
oxide and coke (pure carbon). If 25.0 kilograms of pure Fe2O3 is used, how many kilograms of
iron can be produced? The reaction is: Fe2O3 + 3 C  2 Fe + 3 CO
16. The average human requires 120.0 grams of glucose (C6H12O6) per day. How many grams of
CO2 (in the photosynthesis reaction) are required for this amount of glucose?
The photosynthetic reaction is: 6 CO2 + 6 H2O  C6H12O6 + 6 O2
17. Given the reaction: 4 NH3 (g) + 5 O2 (g)  4 NO (g) + 6 H2O (l)
What is the total number of moles of products formed when 1.20 mole of ammonia reacts?
18. C6H12O6 (aq)  2 C2H5OH (aq) + 2 CO2 (g)
a. How many moles of CO2 are produced when 0.400 mol of C6H12O6 reacts in this fashion?
b. How many grams of C6H12O6 are needed to form 7.50 g of C2H5OH?
c. How many grams of CO2 form when 7.50 g of C2H5OH are produced?
19. Fe2O3 (s) + CO (g)  Fe(s) + CO2 (g) (unbalanced!)
a. Calculate the number of grams of CO that can react with 0.150 kg of Fe 2O3
b. Calculate the mass of Fe and the mass of CO2 formed when 0.150 kg of Fe2O3 reacts
20. A 2.50-g sample of bronze, an alloy of copper and tin, was dissolved in sulfuric acid. The copper in the alloy
reacts with sulfuric acid as shown by the following balanced reaction.
Cu + 2H2SO4 → Cu2+ + SO2 + 2H2O + SO42–
Adding KI produces CuI and triodide, I3–
2Cu2+ + 5 I– → 2CuI + I3–
Finally, titrating the I3– with S2O32–
I3– + 2S2O32– → 3 I– + S4O62–
provides an indirect method for determining the amount of Cu in the original sample. Calculate the percentage,
by mass, of copper in a sample of bronze if 31.5 mL of 1.00 M S2O32– is consumed in the titration.
21. Iron reacts with O2 to produce two different oxides, Fe2O3 or Fe3O4. If 167.6 g of Fe reacts completely with
excess O2, producing 231.6 g of product, which oxide was formed?
22. If 6.80 g of PH3 and 6.80 g of O2 are combined according to the (unbalanced) reaction:
___ PH3 + ___ O2 → ___ P4O10 + ___ H2O
a) Identify the limiting reagent and the excess reactant.
b) How many grams of P4O10 will be formed?
c) How many grams of the excess reagent will remain unreacted?
d) Only 6.58 g of P4O10 are formed in the experiment. What is the percent yield?
23. Assume that two experiments are performed on the chemical reaction given below.
2Br– + Cl2 → Br2 + 2Cl–
–2
Experiment 1: 100.0 mL of 1.00×10 M Br– is added to 50.00 mL of 2.00×10–2 M Cl2
Experiment 2: 100.0 mL of 2.00×10–2 M Br– is added to 50.00 mL of 1.00×10–2 M Cl2
Solutions of Br–, Cl2, and Cl– are colorless, but a solution of Br2 is red. If the reaction between Br– and Cl2
always goes to completion, which of the following observations is correct? Explain.
Observation A: The solution in experiment 1 will be a darker red.
Observation B: The solution in experiment 2 will be a darker red.
Observation C: The solutions will be the same shade of red.
24. A process to produce aluminum from aluminum oxide has an 85.0% yield. How much
aluminum will be produced from a reacting 700.0 kg of aluminum oxide to produce Al?
The reaction is : __ Al2O3 + __ H2  __ Al + __ H2O