E-19 Single Replacement Reaction
DATA TABLE:
LETTER OF YOUR GROUP: ________
1
Mass of copper wire (before)
2
Mass of vial & lid containing AgNO3
3
Mass of empty beaker
Name Partner(s) Partner(s) Period -
4
Mass of empty vial & lid
5*
6
7
Mass of AgNO3 crystals - calculated (#2 - #4)
Volume of water added
Mass of watch glass and copper coil (after)
8
9
Mass of watch glass
Mass of copper coil (after) - calculated (#7- #8)
10*
Mass of copper coil reacted - calculated (#1 - #9)
11
Mass of 1 sheet of filter paper
12
13*
Mass of beaker, filter paper, and silver residue
Mass of silver produced - calculated (#12 - #11 - #3)
14*
Mass of Cu(NO3)2 produced – calculated (#5 + #10 - #13)
______
______
______
* Data # 5, 10, 13, & 14 will be the ONLY data used in the following calculations.
Calculations: (Calculation work required for credit (Staple a separate sheet to the back of this
paper.)!!! Be sure to express your calculations using the correct number of significant figures!!!)
1.
2.
Calculate the number of moles (from grams in the Data Table) of:
a.
copper (Cu) that reacted (Data #10);
Cu =
b.
silver nitrate (AgNO3) in the vial at the start of the lab (Data #5); AgNO3 =
c.
silver (Ag) obtained (Data #13);
d.
copper (II) nitrate, Cu(NO3)2, produced (Data #14).
Ag =
Cu(NO3)2 =
Determine 4 ratios using the numbers obtained in Calculation #1
(Don’t forget to divide! Please use correct significant figures! There are
NO UNITS in ratios!).
a.
moles of copper reacted/ moles of copper reacted;
Cu =
b.
moles of silver nitrate / moles of reacted copper;
c.
moles of silver / moles of reacted copper;
d.
moles of copper (II) nitrate / moles of reacted copper.
AgNO3 =
Ag =
Cu(NO3)2 =
Questions for DAY TWO:
6. Using the Basic Molarity Equation, calculate the molarity (M) of the silver nitrate solution that
you made on Day One.
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Questions for DAY THREE:
Go and find two people (or pairs) who had a different letter (A, B, or C) than you did, and fill in the
following information from their data tables in the appropriate column. Record your own data in
the column for your letter. *In the last row, use the terms “pale”, “dark”, or “medium” to
describe the 3 solutions, based on your memory from Day Two.
Group A
Group B
Group C
Mass of AgNO3 used
(Data #5)
Mass of Cu reacted
(Data #10)
Mass of Ag produced
(Data #13)
Mass of Cu(NO3)2
produced (Data #14)
Molarity of AgNO3
(from Day 2 Question #6)
Intensity of blue color in
Cu(NO3)2 solution*
(from Day 2 Question #2)
Using the data above, answer the following questions. For Questions #1-4, circle ONE answer,
then write a brief explanation/support of your answer.
1.
How does the “mass of AgNO3 used” relate to the “mass of Cu reacted”?
Direct
2.
None
Inverse
None
How does the “mass of AgNO3” relate to the “molarity of AgNO3”?
Direct
5.
Inverse
How does the “mass of Cu reacted” relate to the color intensity of the Cu(NO3)2 solution in the
beaker on Day Two?
Direct
4.
None
How does the “mass of AgNO3 used” seem to relate to the “mass of Ag produced” and the
“mass of Cu(NO3)2 produced”?
Direct
3.
Inverse
Inverse
None
FILL IN THE BLANKS IN THIS SENTENCE (Use words like “more” or “less”.)
The more of one reactant you use in a chemical reaction, the _______________ of the other
reactant will be needed; meanwhile you will produce ___________________ of the products.
The amount of reactants present becomes ___________________ as the reaction progresses,
and the amount of products becomes ____________________.
6.
If the “mass of AgNO3 used” were 3.00 grams, what would you expect the “mass of Ag
produced” to be (You can give a range of values.)?
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QUESTIONS THAT DO NOT DEPEND ON THE CHART ON THE PREVIOUS PAGE!
1.
Using the ratio results obtained in Calculation #2, write the whole number coefficients on the
line above the letter that corresponds to that chemical in the equation below:
1
2.
mole Cu + ___ mole(s) AgNO3 
(a)
(b)
___ mole(s) of Ag + ___ mole(s)of Cu(NO3)2
(c)
(d)
Balance the following chemical reaction using coefficients (like we learned in E-20)
___ Cu + _____ AgNO3  ______ Ag + _______ Cu(NO3)2
3.
How do the numbers you wrote in for Questions #1 & #2 above compare? Should they be the
same?
4.
What were the two reactants in this reaction? (Give their chemical formulas and names)
5.
What were the two products of this reaction? (Give their chemical formulas and names)
6.
Look at the chemical equation for this reaction. In terms of the arrangement of the atoms, what
has happened to the two metals, Cu and Ag, involved in this reaction?
7.
Look up and write definitions for “limiting reactant” and “excess reactant.” Based on your
observations of this experiment, identify which is the “limiting reactant” and which is the
“excess” reactant.
8.
What happens to the molarity of the silver nitrate solution (a reactant) as the reaction progresses?
(Hint: How much silver nitrate, a reactant, is left when the reaction has concluded?)
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