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HL IB Chemistry Unit 1.2
Unit 1.4
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Cards (132)
Why is it important to identify the limiting reactant?
It determines the
maximum product
formed
What is needed to convert moles of product to grams?
The
molar mass
of the product
What is the molar mass of
H
2
O
H_{2}O
H
2
O
?
18 g/mol
How does the limiting reactant affect product formation?
It determines the
maximum amount
of product
How does analyzing percent yield help chemists?
Evaluates
chemical reaction
efficiency
Identifies areas for improvement
Enhances understanding of
reaction dynamics
What happens to the reaction after the limiting reactant is consumed?
The reaction stops, regardless of other
reactants
What is a limiting reactant in a chemical reaction?
The substance
completely
used up first
What is the first step to identify the limiting reactant?
Convert amounts to
moles
What is the significance of identifying the limiting reactant in a chemical reaction?
It helps predict the amount of
product
formed
What is the role of a limiting reactant in a chemical reaction?
Determines the
maximum amount of product
Runs out first,
halting the reaction
Influences the
yield of the reaction
In the equation 2H₂ + O₂ → 2H₂O, what is the mole ratio of H₂ to O₂ if you have 2 moles of H₂ and 1 mole of O₂?
2:1
What indicates which reactant is limiting in a chemical reaction?
The smaller
mole ratio
relative to its
coefficient
How many grams of
H
2
O
H_{2}O
H
2
O
are produced from 3 moles?
54
grams
What does the theoretical yield represent in a chemical reaction?
The
maximum
possible product from reactants
What is percent yield in a chemical reaction?
Measure of actual product vs.
theoretical yield
In the reaction
2
H
2
+
2H_{2} +
2
H
2
+
O
2
→
2
H
2
O
O_{2} \to 2H_{2}O
O
2
→
2
H
2
O
, which reactant is limiting if there are 3 moles of
H
2
H_{2}
H
2
and 2 moles of
O
2
O_{2}
O
2
?
H
2
H_{2}
H
2
is the
limiting
reactant
In the
reaction
2
H
2
+
2H_{2} +
2
H
2
+
O
2
→
2
H
2
O
O_{2} \to 2H_{2}O
O
2
→
2
H
2
O
, what does the actual yield represent?
The amount of water produced in the reaction
What are the steps to calculate percent yield?
Recall the
percent yield formula
.
Identify
actual and theoretical yields
.
Substitute
values into the formula
.
Calculate the percent yield.
What is the formula for percent yield?
Percent Yield
=
\text{Percent Yield} =
Percent Yield
=
Actual Yield
Theoretical Yield
×
100
\frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100
Theoretical Yield
Actual Yield
×
100
What does a
percent yield
of
92.6%
indicate when making cookies?
You obtained 92.6% of expected cookies
What is a limiting reactant?
An
ingredient
that runs out first
If the actual yield is 50 grams and theoretical yield is 54 grams, what is the percent yield?
92.6
%
92.6\%
92.6%
What does a high percent yield suggest about a chemical reaction?
Efficient use of
reactants
and minimal waste
What is a mole ratio?
The ratio of
moles
of reactants to products
What does it mean if neither reactant is limiting in a reaction?
Both reactants are present in
required
amounts
How does the percent yield reflect the efficiency of a chemical reaction?
It compares actual production to
theoretical
expectations
What is the theoretical yield in stoichiometry?
The
maximum
amount of product possible
What does a low percent yield indicate?
Potential issues like
incomplete reaction
If you have 2 moles of H₂ and 0.5 moles of O₂, what is the mole ratio of H₂ to O₂?
4:1
What does percent yield indicate in a chemical reaction?
Efficiency
of reactant use and waste
What is the formula to calculate percent yield?
Percent Yield
=
\text{Percent Yield} =
Percent Yield
=
Actual Yield
Theoretical Yield
×
100
\frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100
Theoretical Yield
Actual Yield
×
100
How do you substitute values into the percent yield formula?
Percent Yield
=
\text{Percent Yield} =
Percent Yield
=
50
g
54
g
×
100
\frac{50 \text{ g}}{54 \text{ g}} \times 100
54
g
50
g
×
100
How do you compare mole ratios in a balanced equation?
By comparing them to
reactants' mole ratios
Why do we convert amounts to moles in limiting reactant identification?
To use
mole ratios
in the equation
What factors can influence the
actual yield
in a
reaction
?
Incomplete reaction, side reactions, or loss
What are the steps to calculate theoretical yield using stoichiometry?
Identify the
limiting reactant
.
Use the
mole ratio
from the balanced equation.
Convert moles of product to grams using
molar mass
.
How many moles of
H
2
O
H_{2}O
H
2
O
can be produced from 3 moles of
H
2
H_{2}
H
2
in the reaction?
3 moles of
H
2
O
H_{2}O
H
2
O
What does a 92.6% yield suggest about the hydrogen and oxygen process?
It indicates a
relatively efficient process
In the
reaction
2H₂
+ O₂ →
2H₂O
, which reactant is
limiting
?
Hydrogen (H₂)
What is the first step in calculating theoretical yield?
Identify the
limiting reactant
See all 132 cards
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