Save
AQA GCSE Chemistry
3. Quantitative chemistry
3.3 Yield and atom economy of chemical reactions
Save
Share
Learn
Content
Leaderboard
Share
Learn
Cards (31)
What does yield refer to in chemistry?
Amount of product obtained
Percentage yield is calculated as (Actual Yield / Theoretical Yield) ×
100
Arrange the steps to calculate the percentage yield:
1️⃣ Determine the actual yield
2️⃣ Calculate the theoretical yield
3️⃣ Divide the actual yield by the theoretical yield
4️⃣ Multiply by 100
A high atom economy minimizes waste and promotes sustainability.
True
A higher percentage yield indicates a more efficient reaction.
True
What is the formula for calculating percentage yield in chemistry?
P
e
r
c
e
n
t
a
g
e
Y
i
e
l
d
=
Percentage \, Yield =
P
erce
n
t
a
g
e
Yi
e
l
d
=
A
c
t
u
a
l
Y
i
e
l
d
T
h
e
o
r
e
t
i
c
a
l
Y
i
e
l
d
×
100
%
\frac{Actual \, Yield}{Theoretical \, Yield} \times 100\%
T
h
eore
t
i
c
a
l
Yi
e
l
d
A
c
t
u
a
l
Yi
e
l
d
×
100%
Match the type of yield with its definition:
Actual Yield ↔️ Amount obtained experimentally
Theoretical Yield ↔️ Maximum possible amount
Percentage Yield ↔️ (Actual Yield / Theoretical Yield) × 100%
Atom economy
measures the proportion of reactant atoms that end up in the desired
product
The theoretical yield is the amount of product obtained in the experiment.
False
Atom economy focuses on the waste produced in a reaction, while
yield
focuses on the product obtained.
True
What is the theoretical yield in chemistry?
Maximum possible product
Match the type of yield with its definition:
Actual Yield ↔️ Amount of product obtained experimentally
Theoretical Yield ↔️ Maximum possible amount of product
Percentage Yield ↔️ Ratio of actual to theoretical yield
What is the formula for atom economy?
({\text{Mass of Desired Product} \over \text{Total Mass of Reactants}}) \times 100\%</latex>
If a reaction could theoretically produce 25 grams of product, but only 20 grams are obtained, the percentage yield is
80
%
Percentage yield is calculated as (Actual Yield / Theoretical Yield) ×
100
A higher percentage yield indicates a more efficient
chemical reaction
.
True
A high atom economy indicates that most reactants are converted into the
desired
product.
True
How is percentage yield calculated using actual yield and theoretical yield?
P
e
r
c
e
n
t
a
g
e
Y
i
e
l
d
=
Percentage \, Yield =
P
erce
n
t
a
g
e
Yi
e
l
d
=
A
c
t
u
a
l
Y
i
e
l
d
T
h
e
o
r
e
t
i
c
a
l
Y
i
e
l
d
×
100
%
\frac{Actual \, Yield}{Theoretical \, Yield} \times 100\%
T
h
eore
t
i
c
a
l
Yi
e
l
d
A
c
t
u
a
l
Yi
e
l
d
×
100%
What is the key difference between yield and atom economy?
Yield measures product quantity, atom economy measures reactant use
Order the aspects by their benefits of high yield and high atom economy:
1️⃣ Cost reduction
2️⃣ Sustainability
3️⃣ Waste minimization
The actual yield is the amount of product obtained from the
experiment
Incomplete reactions can affect the yield of a chemical reaction.
True
Atom economy measures how much of the reactants' atoms end up in the desired
product
What is the formula for calculating percentage yield?
(
Actual Yield
Theoretical Yield
)
×
100
%
({\text{Actual Yield} \over \text{Theoretical Yield}}) \times 100\%
(
Theoretical Yield
Actual Yield
)
×
100%
What are the three types of yield in chemistry?
Actual, theoretical, percentage
In the percentage yield formula,
Actual Yield
refers to the amount of product obtained
experimentally
What are three factors that can affect the yield of a chemical reaction?
Incomplete reactions, side reactions, losses during isolation
What is the formula for calculating atom economy?
A
t
o
m
E
c
o
n
o
m
y
=
Atom \, Economy =
A
t
o
m
E
co
n
o
m
y
=
M
a
s
s
o
f
D
e
s
i
r
e
d
P
r
o
d
u
c
t
T
o
t
a
l
M
a
s
s
o
f
R
e
a
c
t
a
n
t
s
×
100
%
\frac{Mass \, of \, Desired \, Product}{Total \, Mass \, of \, Reactants} \times 100\%
T
o
t
a
l
M
a
ss
o
f
R
e
a
c
t
an
t
s
M
a
ss
o
f
Des
i
re
d
P
ro
d
u
c
t
×
100%
Match the yield component with its description:
Actual Yield ↔️ Amount obtained from experiment
Theoretical Yield ↔️ Maximum amount obtainable
Atom economy is calculated as the mass of the desired product divided by the total mass of the
reactants
What are three benefits of high yield and high atom economy in the chemical industry?
Cost reduction, sustainability, waste minimization