Limiting Reactant and Theoretical Yield

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

Tags

NGSS.HS-PS1-7

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

Tags

NGSS.HS-PS1-7

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

Tags

NGSS.HS-PS1-7

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

Tags

NGSS.HS-PS1-7

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

Tags

NGSS.HS-PS1-7

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%

Tags

NGSS.HS-PS1-7

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.

Tags

NGSS.HS-PS1-7