1. ____ N2 + ____ H2 ____ NH
a)
N2 / H2
b)
N2 / NH3
c)
H2 / NH3
d)
6.2 moles of N2 requires _________moles H2
e)
3.5g of N2 will produce _________g. of NH3
f)
How much H2 is required to produce 4.8 g of NH3
2. ____ H2 + ____ S8  _____ H2S
a)
H2 / H2S
b)
H2 / S8
c)
H2S / S8
d)
17 moles of H2 will produce _________moles of H2S
e)
68.2 grams of S8 will produce ________grams of H2S
3. ____H2 + ____O2  ____H2O
a)
H2 / H2O
b)
O2 / H2O
c)
25 moles of H2 will produce ________moles of H2O
d)
16g of O2 will produce __________grams of H2O
4. ____Li3N + ____H2O  ____NH3 + ____LiOH
a)
Li3N / H2O
b)
LiOH / H2O
c)
8 moles of H2O requires ________moles of Li3N
d)
3.2 grams of H2O will produce _________grams of Li3N
1
5. ____Sb2O3 + ____C  ____Sb + ____CO
a)
Sb2O3/CO
b)
C/Sb
c)
5 moles of Sb2O3 will produce ________moles of CO
d)
125g of C will produce __________grams of Sb
2K(ClO3)  2KCl + 3O2
1. How many moles of oxygen are produced when 3.0 moles of potassium chlorate decompose completely?
2. How many grams of K(ClO3) were needed to produce 5 grams of O2?
Use the reaction of butane (C4H10) undergoing combustion to answer questions 4-6.
2C4H10(l) + 13O2(g)  8CO2(g) + 10H2O(l)
3. How many moles of CO2 are produced when 88 moles of O2 are used?
4. How many moles of water are needed when 10 moles of C4H10 used?
5. 12 moles of CO2 were made. How many moles of O2 were needed?
2
Moles to Grams Conversion
What are the molecular weights of the following compounds?
1. NaOH
4. Mn2Se7
2. H3PO4
5. MgCl2
3. H2O
6. (NH4)2SO4
7. Given the following equation: 2 NaClO3 → 2 NaCl + 3 O2. With 12.00 moles of NaClO3 how many
grams of O2 will produce?
8. For the reaction C + 2H2 → CH4, how many grams of hydrogen are required to produce 0.6 moles of
methane, CH4 ?
9. Balance the reaction: _____Cl2 + ____KBr → _____KCl +_____ Br2. Calculate how many grams of
potassium chloride are produced from 4.3 moles of potassium bromide?
10. Balance the reaction: ____Zn +____ O2 → ____ZnO. Calculate how many grams of zinc oxide can be
produced from 7.3 moles of oxygen?
3
Grams to Mole Conversion
1. Given the following equation: 2 NaClO3 → 2 NaCl + 3 O2. With 12 g of NaClO3 how many moles of
O2 will produce?
2. For the reaction C + 2H2 → CH4, how many moles of hydrogen are required to produce 0.6 grams of
methane, CH4 ?
3. Balance the reaction: _____Cl2 + ____KBr → _____KCl +_____ Br2. Calculate how many moles of
potassium chloride are produced from 4.3 grams of potassium bromide?
4. Balance the reaction: ____Zn +____ O2 → ____ZnO. Calculate how many moles of zinc oxide can be
produced from 7.3 grams of oxygen?
4
Grams to Grams Conversion
1. For the reaction C + 2H2 → CH4, how many grams of hydrogen are required to produce 145 grams of
methane, CH4 ?
2. For the reaction 2HNO3 + Mg(OH)2 → Mg(NO3) 2 + 2H2O, how many grams of magnesium nitrate are
produced from 981 grams of nitric acid, HNO3 ?
3. For the reaction Cl2 + 2KBr → 2KCl + Br2, how many grams of potassium chloride are produced from
113 g of chlorine?
4. Balance the reaction: _____Zn +_____ O2 → _______ZnO, how many grams of zinc oxide can be
produced from 2.75 g of oxygen?
Balance the reaction and use the equation to answer questions 5-8.
_____C2H2 + ____O2 → _____CO2 + ______H2O
5. How many grams of water are produced from 100 grams of oxygen?
6. How many grams of water are produced from 100 grams of acetylene (C2H2)?
7. What is the limiting reagent for the production of water?
5
Limiting Reactant
8. Balance:
C3H8
+ O2

CO2
+
H2O
a) If you start with 14.8 g of C3H8 and 3.44 g of O2, determine the limiting reagent
b) determine the number of moles of carbon dioxide produced
c) determine the number of grams of H2O produced
d) determine the number of grams of excess reagent left
9. Given the following equation:
Al2(SO3)3 + 6 NaOH  3 Na2SO3
+ 2 Al(OH)3
a) If 10.0 g of Al2(SO3)3 is reacted with 10.0 g of NaOH, determine the limiting reagent
b) Determine the number of moles of Al(OH)3 produced
c) Determine the number of grams of Na2SO3 produced
d) Determine the number of grams of excess reagent left over in the reaction
5. Given the following equation:
Al2O3
+ Fe  Fe3O4
+
Al
a) If 25.4 g of Al2O3 is reacted with 10.2 g of Fe, determine the limiting reagent
b) Determine the number of moles of Al produced
c) Determine the number of grams of Fe3O4 produced
d) Determine the number of grams of excess reagent left over in the reaction
6
Fizzy Drink Activity
Purpose: _________________________________________________________________________
I.
What is the molar mass of citric acid, H3C6H5O7? Round to the nearest whole number.
H=
g/mol
Show your calculations for molar mass here:
C=
g/mol
O=
g/mol
Molar mass of H3C6H5O7 = ____________________________
Part 1
Trial Ingredients
Observations
Taste
1.
¼ Dixie cupful Kool-Aid®
2.
¼ Dixie cupful of KoolAid® + 0 .5 g Citric Acid
3.
¼ Dixie cupful of KoolAid® + 0.5 g Baking soda
(sodium bicarbonate,
NaHCO3)
Summarize the conclusions from the group discussion in the space below:
_____________________________________________________________________________________
Part 2
1. Write the chemical equation for this reaction.
__________
____________
citric acid
+
baking soda

Na3C6H5O7
sodium citrate
2. Determine if the equation is balanced in the table below:
Element
# of atoms on the reactant
side
H
______
+ water
____________
+ carbon dioxide
# of atoms on the product
side
C
O
Na
3. Is the reaction balanced? If not, rewrite the equation below and add coefficients as needed.
4. Check with the teacher before continuing. Teacher initials: ______________
7
Part 3
THE BIG IDEA: You will be given exactly _____ grams of citric acid. You need to calculate how many grams
of baking soda (NaHCO3) should be added to make a fizzy Kool-Aid® drink that is “just right”.
You now have your recipe for your Fizzy Drink:
_______ g of citric acid (H3C6H5O7)
_______ g of baking soda (NaHCO3)
Before continuing, have the teacher check your recipe. Teacher initials: ________________
Procedure
1. Fill a Dixie cup with Kool-Aid®. Pour the Kool-Aid® from the Dixie cup into a larger cup (to prevent
bubble-overs).
2. Now add your calculated amounts of citric acid (H3C6H5O7) and baking soda (NaHCO3) in the recipe
above to the Kool-Aid®.
3. Mix and taste (pour into several small cups if more than one person wants to try it).
Part 4
1. How did your drink turn out?
2. How could you modify your recipe to make it better?
3. If you have 10.0 grams of baking soda (NaHCO3) with enough citric acid (H3C6H5O7)
how many moles of carbon dioxide can you produce? (Use balanced equation).
4. Refer to the moles of CO2 produced in question 3. Which reactant, citric acid (H3C6H5O7) or baking
soda (NaHCO3), produced less CO2?
5. If you mixed 7 grams of each reactant in a container, would both of them be used up completely? How
do you know?
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