Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
NUCLEAR CHEMISTRY:
Complete the following table:
Alpha
Beta
or
or
Charge
Relative
mass
Symbol
Stopped by
In the following reactions, identify the type of decay as alpha, beta or gamma.
1.
14
6C
2.
228
3.
40
86
147N +
Rn 
18Ar

0
0
4
-1e
2He
y+
0
+
_______________________________
224
40
18
84Po
_______________________________
Ar
_______________________________
Balancing Nuclear Decay Equations:

Predict the product or reactant of the following nuclear reactions.
4.
226
88
Ra 
4
2He
+
5. ______________ 
6.
1
1

H+
3
1
_______________
0
+1e
+
53
25Mn
H  _______________
Fission and Fusion:
Nuclear Fusion:
o
Two smaller nuclei are coming together to form one larger, more stable nucleus.
o
Examples of Sun and Hydrogen bomb.
Nuclear Fission:
o
One large nuclei splits into two smaller and more stable nuclei.
Gama
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
o Examples of nuclear power plant and atomic bomb.
7. What is it called when a nucleus splits apart and releases massive amounts of energy?
____________________________________________
8. Which releases more energy fission or fusion?
____________________________________________
MOLE CONVERSIONS:
 To calculate Molar Mass
Amount of
Na atoms in
the formula
Mass of Na from
periodic table
EXAMPLE: NaCl
Molar mass of NaCl = (1 X 23.0 g/mole) + (1 X 35.5 g/mole) = 58.5 g/mole
Practice: Determine the molar mass for the following compounds:
9. Al(CH3CO2)3
10. C6H8O6
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
 Percent Composition:
How to Calculate % Composition Steps:
1. Calculate the molar mass of the compound.
2. Divide the total mass of the element by the molar mass of the compound.
3. Multiply step 2 by 100%.
Example: Find the percent of oxygen in KMnO4
Amount of
Na atoms in
the formula
Mass of Na from
periodic table
Step 1:K: (1 X 39.1 g/mol) = 39.1 g/mol
Mn: (1 X 54.9 g/mol) = 54.9 g/mol
O: (4 X 16.0 g/mol) = 64.0 g/mol
Molar Mass = 39.1 g/mol + 54.9 g/mol + 64.0 g/mol = 158.0 g/mol
Step 2: 64.0 g/mol ÷ 158.0 g/mol = 0.41
Step 3: 0.41 X 100% = 41%
Practice: Determine the percentage composition of each in the compounds below.
11. Al(CH3CO2)3
Al=
___________________
C=
___________________
H=
___________________
O=
___________________
12. C6H8O6
C=
___________________
H=
___________________
O=
___________________
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)

Mole Conversions:

To calculate from grams to moles
𝑔𝑖𝑣𝑒𝑛 (𝑔)
1 𝑚𝑜𝑙
∗
= ____𝑚𝑜𝑙𝑒𝑠
Conversion(s) needed:
1
𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 (𝑔)
1 mol = molar mass

To calculate from moles to grams
Molar Mass = 1 mol
𝑔𝑖𝑣𝑒𝑛 (𝑚𝑜𝑙𝑒𝑠) 𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 (𝑔)
∗
= ____𝑔𝑟𝑎𝑚𝑠
1
1 𝑚𝑜𝑙𝑒
Example:
How many moles are in 125 grams of MgCl2?
Conversion(s) needed:
1 mol of MgCl2= 95.3 g/mol
125 𝑔𝑟𝑎𝑚𝑠
1 𝑚𝑜𝑙𝑒
∗
= 1.3 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑀𝑔𝐶𝑙2
1
95.3 𝑔𝑟𝑎𝑚𝑠
Practice:
Solve the following. Round your answers to the correct number of significant figures.
13. How many moles are in 125 grams of MgCl2?
14. How many grams are in 1.91 moles of Zn?
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
To calculate from particles (atoms, formula units, molecules) to moles
𝑔𝑖𝑣𝑒𝑛 (𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠)
1
∗
1 𝑚𝑜𝑙
6.02 𝑋 1023 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠
= ____𝑚𝑜𝑙𝑒𝑠
Conversion(s) needed:
1 mol = 6.02 X 1023 particles (molecules, atoms)
6.02 X 1023 particles (molecules, atoms) = 1 mol
To calculate from moles to particles (atoms, formula units, molecules)
𝑔𝑖𝑣𝑒𝑛 (𝑚𝑜𝑙𝑒𝑠) 6.02 𝑋 1023 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠
∗
= ___𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠
1
1 𝑚𝑜𝑙𝑒
Example:
How many moles are in 1.5 x 1024molecules of CO2?
1.5 𝑥 1024 𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠
1 𝑚𝑜𝑙
∗
1
6.02 𝑋 1023 𝑚𝑜𝑙𝑒𝑐𝑢𝑙𝑒𝑠
= 2.5 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝐶𝑂2
Conversion(s) needed:
6.02 X 1023 particles (molecules, atoms) = 1 mol**On the formula Chart**
Practice:
Solve the following. Round your answers to the correct number of significant figures.
15. How many moles are in 1.5 x 1024molecules of CO2?
16. How many formula units are in 3.43 moles of LiF?
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
17. How many atoms are in 1 mole of potassium?
To calculate from particles (atoms, formula units, molecules) to grams
𝑔𝑖𝑣𝑒𝑛 (𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠)
1 𝑚𝑜𝑙
𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 (𝑔)
∗
∗
23
1
6.02 𝑋 10 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠
1 𝑚𝑜𝑙
= _____𝑔𝑟𝑎𝑚𝑠
Conversion(s) needed:
1 mol = 6.02 X 1023 particles
1 mole = molar mass
To calculate from grams to particles (atoms, formula units, molecules)
𝑔𝑖𝑣𝑒𝑛 (𝑔)
1 𝑚𝑜𝑙
6.02 𝑋 1023 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠
∗
∗
1
𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 (𝑔)
1 𝑚𝑜𝑙
= _______𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠
Conversion(s) needed:
Example:
Convert 6.52 X 10
25
atoms of gold to grams.
1 mol = 6.02 X 1023 particles
1 mole = 196.967 g/mol
6.52 𝑥 1025 𝑎𝑡𝑜𝑚𝑠
1 𝑚𝑜𝑙
196.967 𝑔
∗
∗
1
6.02 𝑋 1023 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠
1 𝑚𝑜𝑙
= 21332
Practice:
Solve the following. Round your answers to the correct number of significant figures.
18. Convert 6.52 X 1025 atoms of gold to grams.
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
19. Convert 24.5 grams of K3PO4 to formula units.
20. Convert 51 grams of O2 to molecules.

Empirical Formulas (lowest whole number ratio):
How to calculate empirical formulas steps:
*Assume 100 gram sample if given percentages  simply replace % for grams
*If not, use grams.
1. Convert grams to moles.
2. Divide by the smallest number of moles.
3. If the numbers aren’t whole numbers, the multiply by a common number. For example, if the answer is
1.25 multiply by 4.
4. The whole numbers become the subscripts in the formula. Write the formula in the order the elements
were given in the problem.
Practice:
21. What is the empirical formula of the compounds below?
a) 68.4% chromium, 31.6% oxygen
b) 74.0% carbon, 8.7% hydrogen and the rest nitrogen
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
 Molecular Formulas (true formulas):
How to calculate molecular formulas steps:
1. Calculate the molar mass of the empirical formula. If the empirical formula is not provided, solve for it
first.
2. Divide the molar mass of the molecular formula (given in the problem) by the molar mass of the
empirical formula. This must be a whole number.
3. Multiply the answer from step 2 by each subscript in the empirical formula.
Practice:
Determine the molecular formulas of the compounds below.
22. A compound is 43.7% Phosphorus and 56.3% Oxygen. The molar mass of the compound is 284 g/mole.
Calculate the molecular formula of the compound.
23. A compound with an empirical formula of CFBrO has a molar mass of 254.7 grams per mole. Calculate the
molecular formula of the compound.
STOICHIOMETRY:
**Remember to ALWAYS start with a balanced chemical equation!!!**
Mole-Mole Conversions:
To calculate from moles to moles
Conversion(s) needed:
Xmol given = X mole find (X
is from the balanced eq.)
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
𝑥 𝑚𝑜𝑙 𝑜𝑓
𝑓𝑖𝑛𝑑
𝑔𝑖𝑣𝑒𝑛 (𝑚𝑜𝑙)
𝑤𝑎𝑛𝑡
∗
= _____𝑚𝑜𝑙𝑒𝑠
1
𝑥 𝑚𝑜𝑙 𝑜𝑓 𝑔𝑖𝑣𝑒𝑛
Example:
How many moles of sodium oxide are produced when 3.90 moles of sodium combine with oxygen gas?
__Na + __O2___Na2O
Balance
first!!
3.90 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎 2 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎2 𝑂
∗
= 1.95 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑁𝑎2 𝑂
1
4 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎
4Na + 1O2
Practice:
2Na2O
Balance first!!
Solve the following round your answer to the correct number of significant figures.
24. Given: ____NH3 + ____NO  ____N2 + ____H2O
a. How many moles of NO are needed to react with 15.0 moles of NH3?
b. How many moles of water are produced if 2.45 moles of NO react with NH3?
Mole-Mass Conversions:
To calculate from moles to mass
Conversion(s) needed:
Xmol given = X mole find (X is from the balanced eq.)
1 mole = molar mass
𝑥 𝑚𝑜𝑙 𝑜𝑓
𝑓𝑖𝑛𝑑
𝑔𝑖𝑣𝑒𝑛 (𝑚𝑜𝑙)
𝑤𝑎𝑛𝑡
∗
∗
1
𝑥 𝑚𝑜𝑙 𝑜𝑓 𝑔𝑖𝑣𝑒𝑛
= ___𝑔𝑟𝑎𝑚𝑠
Example:
𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑜𝑓
1 𝑚𝑜𝑙 𝑜𝑓
𝑓𝑖𝑛𝑑
𝑤𝑎𝑛𝑡
𝑓𝑖𝑛𝑑
𝑤𝑎𝑛𝑡
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
How many grams of sodium oxide are produced when 3.90 moles of sodium combine with oxygen gas?
__Na + __O2___Na2O
Conversion(s) needed:
Balance first!!
4mol Na = 2 mole Na2O
4Na + 1O2
2Na2O
1 mole Na2O= 62.0 grams Na2O
3.90 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎 2 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎2 𝑂 62. 𝑂 𝑔 𝑁𝑎2 𝑂
∗
∗
1
4 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎
1 𝑚𝑜𝑙𝑒 𝑁𝑎2 𝑂
= 121 𝑔𝑟𝑎𝑚𝑠 𝑁𝑎2 𝑂
Practice:
Solve the following round your answer to the correct number of significant figures.
25. Given: ____Hg + ____Br2 ____HgBr2
How many grams of mercury (II) bromide are produced when 3.21 moles of mercury react with bromine gas?
Conversion(s) needed:
Mass-Mole Conversions:
Xmol given = X mole find (X is from the balanced eq.)
To calculate from moles to mass
1 mole = molar mass
𝑥 𝑚𝑜𝑙 𝑜𝑓
𝑓𝑖𝑛𝑑
𝑔𝑖𝑣𝑒𝑛 (𝑔)
1 𝑚𝑜𝑙𝑒 𝑜𝑓 𝑔𝑖𝑣𝑒𝑛
𝑤𝑎𝑛𝑡
∗
∗
1
𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑔𝑖𝑣𝑒𝑛 𝑥 𝑚𝑜𝑙 𝑜𝑓 𝑔𝑖𝑣𝑒𝑛
= _____𝑚𝑜𝑙𝑒𝑠
Example:
How many moles of sodium oxide are produced when 3.90 grams of sodium combine with oxygen gas?
__Na + __O2___Na2O
Balance first!!
4Na + 1O22Na2O
Conversion(s) needed:
4mol Na = 2 mole Na2O
1 mole Na = 23.0 grams Na
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
3.90 𝑔 𝑁𝑎
1 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎
2 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎2 𝑂
∗
∗
1
23.0 𝑔𝑟𝑎𝑚𝑠 𝑁𝑎
4 𝑚𝑜𝑙𝑒 𝑁𝑎
Practice:
Solve the following round your answer to the correct number of significant figures.
26. Given: ____Hg + ____Br2 ____HgBr2
How many moles of bromine gas are required to produce 10.0 g of mercury (II) bromide?
Mass-Mass Conversions:
Conversion(s) needed:
To calculate from moles to mass
Xmol given = X mole find (X is from the balanced eq.)
1 mole = molar mass (given and want/find)
𝑓𝑖𝑛𝑑
𝑓𝑖𝑛𝑑
𝑥 𝑚𝑜𝑙𝑒 𝑜𝑓
𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑜𝑓
𝑔𝑖𝑣𝑒𝑛 (𝑔)
1 𝑚𝑜𝑙𝑒 𝑜𝑓 𝑔𝑖𝑣𝑒𝑛
𝑤𝑎𝑛𝑡
𝑤𝑎𝑛𝑡
∗
∗
∗
= ____𝑔𝑟𝑎𝑚𝑠
𝑓𝑖𝑛𝑑
1
𝑚𝑜𝑙𝑎𝑟 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑔𝑖𝑣𝑒𝑛 𝑥 𝑚𝑜𝑙𝑒 𝑜𝑓 𝑔𝑖𝑣𝑒𝑛
1 𝑚𝑜𝑙𝑒 𝑜𝑓
𝑤𝑎𝑛𝑡
Example:
How many grams of sodium oxide are produced when 3.90 grams of sodium combine with oxygen gas?
__Na + __O2___Na2O
Balance first!!
4Na + 1O2
2Na2O
Conversion(s) needed:
2 mole Na2O = 4 moles Na
1 mole Na = 23.0 grams Na
1 mole Na2O = 62.0 grams Na2O
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
3.90 𝑔 𝑁𝑎 1 𝑚𝑜𝑙𝑒 𝑁𝑎 2 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎2 𝑂 62.0 𝑔 𝑁𝑎2 𝑂
∗
∗
∗
= 5.26 𝑔𝑟𝑎𝑚𝑠 𝑁𝑎2 𝑂
1
23.0 𝑔 𝑁𝑎
4 𝑚𝑜𝑙𝑒𝑠 𝑁𝑎
1 𝑚𝑜𝑙𝑒 𝑁𝑎2 𝑂
Practice:
Solve the following round your answer to the correct number of significant figures.
27. If 59.3 grams of Iron (III) oxide react with carbon monoxide to produce iron and carbon dioxide, how
many grams of carbon dioxide will be produced?
28. If 59.3 grams of Iron (III) oxide react with carbon monoxide to produce iron and carbon dioxide, how
many grams of iron will be produced?
Limiting Reactant
How to solve for a limiting reactant problem?
1. Determine if the problem is a limiting reactant problem, the problem will say“limiting” or you are
given the mass for both reactants.
2. If an equation is written out for you balance the equation, otherwise write and balance the
equation.
3. Set up a mass-mass problem for all of the givens remember to always solve for the same product.
So if you have 2 reactants, you’re doing the problem twice.
4. The limiting reactant is always the reactant that gave you the least amount of product and the excess
is the one that gave you the most.
Practice:
Given: Zn + 2HCl  ZnCl2 + H2
If 56.7 g of zinc reacts with 70.0 grams of hydrochloric acid, determine the limiting reactant. Determine the
maximum amount of zinc chloride that can be made?
1. Determine if the problem is a limiting reactant problem, the problem will say“limiting” or you are
given the mass for both reactants.
Mass is given for both reactants = limiting reactant problem
56.7 grams of zinc & 70.0 grams of hydrochloric acid
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
2. If an equation is written out for you balance the equation, otherwise write and balance the
equation.
Zn + 2HCl  ZnCl2 + H2reaction is balanced
3. Set up a mass-mass problem for all of the givens remember to always solve for the same product.
So if you have 2 reactants, you’re doing the problem twice.
Conversion(s) needed:
1 mole Zn = 1 moles ZnCl2
1 mole Zn = 65.39 grams Zn
1 mole ZnCl2 = 2 moles
1mole ZnCl2 = 136.38 g ZnCl2
1 mole HCl = 36.5 grams HCl
56.7 𝑔 𝑍𝑛 1 𝑚𝑜𝑙𝑒 𝑍𝑛 1 𝑚𝑜𝑙𝑒𝑠 𝑍𝑛𝐶𝑙2 136.38 𝑔 𝑍𝑛𝐶𝑙2
∗
∗
∗
1
65.38 𝑔 𝑍𝑛
1 𝑚𝑜𝑙𝑒𝑠 𝑍𝑛
1 𝑚𝑜𝑙𝑒 𝑍𝑛𝐶𝑙2
= 118.27𝑔𝑟𝑎𝑚𝑠 𝑍𝑛𝐶𝑙2
70.0 𝑔 𝐻𝐶𝑙 1 𝑚𝑜𝑙𝑒 𝐻𝐶𝑙 1 𝑚𝑜𝑙𝑒𝑠 𝑍𝑛𝐶𝑙2 136.38 𝑔 𝑍𝑛𝐶𝑙2
∗
∗
∗
1
36.5 𝑔 𝐻𝐶𝑙
2 𝑚𝑜𝑙𝑒𝑠 𝐻𝐶𝑙
1 𝑚𝑜𝑙𝑒 𝑍𝑛𝐶𝑙2
= 130.78 𝑔𝑟𝑎𝑚𝑠 𝑍𝑛𝐶𝑙2
4. The limiting reactant is always the reactant that gave you the least amount of product.
Limiting reactant since it produces the
smallest number of grams
56.7 𝑔 𝑍𝑛 1 𝑚𝑜𝑙𝑒 𝑍𝑛 1 𝑚𝑜𝑙𝑒𝑠 𝑍𝑛𝐶𝑙2 136.38 𝑔 𝑍𝑛𝐶𝑙2
∗
∗
∗
1
65.38 𝑔 𝑍𝑛
1 𝑚𝑜𝑙𝑒𝑠 𝑍𝑛
1 𝑚𝑜𝑙𝑒 𝑍𝑛𝐶𝑙2
Zn is the limiting reactant
= 118.27𝑔𝑟𝑎𝑚𝑠 𝑍𝑛𝐶𝑙2
118.27 grams is the maximum amount of
ZnCl2 that can be produced
5. The excess reactant is always the reactant that gave you the most amount of product.
Excess reactant since it produces the
largest number of grams
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
70.0 𝑔 𝐻𝐶𝑙 1 𝑚𝑜𝑙𝑒 𝐻𝐶𝑙 1 𝑚𝑜𝑙𝑒𝑠 𝑍𝑛𝐶𝑙2 136.38 𝑔 𝑍𝑛𝐶𝑙2
∗
∗
∗
1
36.5 𝑔 𝐻𝐶𝑙
2 𝑚𝑜𝑙𝑒𝑠 𝐻𝐶𝑙
1 𝑚𝑜𝑙𝑒 𝑍𝑛𝐶𝑙2
= 130.78 𝑔𝑟𝑎𝑚𝑠 𝑍𝑛𝐶𝑙2
Practice:
29. Given: Zn + 2HCl  ZnCl2 + H2
a) If 56.7 g of zinc reacts with 70.0 grams of hydrochloric acid, determine the limiting reactant.
b) What mass of zinc chloride will be produced by the reaction?
c) What mass of excess reagent remains after the reaction?
30. If 52.5 g of iron reacts with 30.0 grams of oxygen, what mass of iron (III) oxide will form?
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)

Percent yield
How to solve for percent yield?
Step 1: If an equation is written out for you balance the equation, otherwise write and balance the
equation.
Step 2: Set up a mass to mass stoichiometry problem to solve for the product stated in the problem. This
is the theoretical yield.
Step 3: Determine the actual yield from the problem, this is the amount produced in the experiment or in a
laboratory setting. Usually given in the problem.
Step 4: Plug in your information in the following equation: % yield = (actual yield/theoretical yield)*100%
Practice:
31. What is the percent yield of aluminum phosphate if a solution containing 33.4 g of sodium
phosphate produced 19.6 g of aluminum phosphate when reacted with excess aluminum chloride
in solution?
___Na3PO4 + ___AlCl3 ___NaCl + ___AlPO4
32. If 84.8 grams of iron (III) oxide produces 57.8 grams of iron, what is the percent yield of
iron in the reaction?
___Fe2O3 + ___CO  ___Fe + ___CO2
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)
Answers:
1. beta
2. alpha
3. gamma
4. 22286Rn
5. 5326 Fe
6. 42 He
7. nuclear fission
8. nuclear fussion
9. 204.0 g/mol
10. 176.0 g/mol
11. Al = 13.2%, C = 35.3%,
H = 4.41%, O = 47.1%
12. C = 40.9%, H = 4.55%,
O = 54.5%
13. 1.31 mol
14. 125 g
15. 2.5 mol
16. 2.06 x 1024 formula
units
17. 6 x 1023 atoms
18. 21,300 atoms
19. 6.95 x 1022 formula
units
20. 9.6 x 1023 molecules
21. a) Cr2O3 b) C5H7N
22. P4O10
23. C2F2Br2O2
24. a) 22.5 mol NO b) 2.45
mol H2O
25. 1,160 g HgBr2
26. 0.0277 mol Br2
27. 49.0 g CO2
28. 41.5 g Fe
29. a) Zinc
b) 118 g
ZnCl2 c) 6.8 g of HCl
in excess
30. 75.1 g of Fe2O3
31. 79.0%
32. 97.5%
Name:_______________________________________________ Date:__________________________Period:_________
CBA REVIEW (Nuclear Chem. Mole Conversions, & Stoichiometry)