Final answer:
The theoretical yield can be calculated using mass-mass calculations based on the reactants' molar ratios, and the percent yield can be determined by comparing the amount of product obtained to the theoretical yield.
Step-by-step explanation:
To determine the theoretical yield and percent yield, we first need to find the limiting reactant. The limiting reactant is the reactant that is completely consumed, limiting the amount of product that can be formed.
Given:
Mass of
�
�
(
�
2
�
3
�
2
)
2
Cu(C
2
H
3
O
2
)
2
= 2.85 g
Mass of
�
�
�
7
�
4
�
�
3
�
NaC
7
H
4
SO
3
N = 6.77 g
Mass of product = 6.17 g
Find the moles of each reactant:
Moles
=
Mass
Molar mass
Moles=
Molar mass
Mass
The molar masses are as follows:
�
�
(
�
2
�
3
�
2
)
2
Cu(C
2
H
3
O
2
)
2
= 181.63 g/mol
�
�
�
7
�
4
�
�
3
�
NaC
7
H
4
SO
3
N = 223.22 g/mol
Moles of
�
�
(
�
2
�
3
�
2
)
2
Cu(C
2
H
3
O
2
)
2
:
Moles
=
2.85
g
181.63
g/mol
Moles=
181.63g/mol
2.85g
Moles of
�
�
�
7
�
4
�
�
3
�
NaC
7
H
4
SO
3
N:
Moles
=
6.77
g
223.22
g/mol
Moles=
223.22g/mol
6.77g
Determine the limiting reactant:
Compare the moles of each reactant. The reactant that produces fewer moles of the product is the limiting reactant.
Calculate the theoretical yield:
Once you determine the limiting reactant, use its moles to find the theoretical yield.
The molar mass of the product
�
�
(
�
7
�
4
�
�
3
�
)
2
(
�
2
�
)
4
⋅
2
�
2
�
Cu(C
7
H
4
SO
3
N)
2
(H
2
O)
4
⋅2H
2
O needs to be known to calculate moles and, subsequently, the theoretical yield.
Calculate the percent yield:
Percent Yield
=
(
Actual Yield
Theoretical Yield
)
×
100
Percent Yield=(
Theoretical Yield
Actual Yield
)×100
Without the molar mass of the product, it's challenging to provide specific numerical values. If you have the molar mass of the product, you can follow these steps to find the theoretical yield and percent yield.