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WorksheetsLimiting Reactant and Theoretical Yield
Total questions: 11
Worksheet time: 6mins
What is the first step in determining the limiting reactant?
Convert the given information about the reactants to moles
Balance the reaction equation
Compare the number of moles of each reactant
Calculate the theoretical yield
What is the purpose of determining the theoretical yield?
To determine the limiting reactant
To convert moles of reactant to grams of product
To compare the actual yield to the theoretical yield
To calculate the percent yield
How do you convert moles of reactant to moles of product?
Using the molecular weight of the reactant
Using the stoichiometric coefficients from the balanced equation
Using the percent yield
Using the limiting reactant
What is the purpose of calculating the percent yield?
To determine the limiting reactant
To convert moles of reactant to grams of product
To compare the actual yield to the theoretical yield
To calculate the theoretical yield
What does a percent yield greater than 100% indicate?
An error in the calculation
A highly effective reaction
An impurity in the product
A theoretical yield greater than expected
What does the theoretical yield represent?
The maximum amount of product that can be made
The actual amount of product obtained
The percent yield of the reaction
The moles of reactant used
Use the balanced equation to answer the following question.
2 FeCl3 + MgO --> Fe2O3 + 3 MgCl2
How many moles of iron chloride (FeCl3) will be produced from 5.50 moles of magnesium oxide (MgO)?
5.50 mol FeCl3
11.0 mol FeCl3
2.25 mol FeCl3
3.67 mol FeCl3
Use the balanced equation to answer the following question:
2 C2H6 + 7 O2 --> 4 CO2 + 6 H2O
Given 8.25 grams of ethane (C2H6), how many moles of carbon dioxide (CO2) will be produced?
0.27 mol CO2
0.55 mol CO2
16.5 mol CO2
0.405 mol CO2
The following reaction is carried out:
2 Na + Cl2 --> 2 NaCl
The mass of the reactant Na is 47.0 g and the mass of the reactant chlorine is 35.0 g. The final mass of NaCl produced is found to be 63.5 g. What is the percent yield of the reaction?
55.1%
74.5%
77.4%
129.1%
What does a percent yield greater than 100% indicate?
The actual yield is equal to the theoretical yield.
The actual yield is less than the theoretical yield.
The actual yield is greater than the theoretical yield.
The percent yield calculation is incorrect.
Given 8.25 grams of ethane (C2H6), how many moles of carbon dioxide (CO2) will be produced?
4.125
8.25
12.375
16.5
