Stoichiometry and Chemical Reactions

This video tutorial explains the concept of limiting reactants using a latte analogy, followed by a detailed walkthrough of balancing chemical equations. It covers the process of identifying the limiting reactant and calculating the theoretical yield. The tutorial also explains how to determine the excess reactant and calculate the percent yield, providing a comprehensive understanding of stoichiometry in chemical reactions.

What is the limiting reactant in a chemical reaction?

• The reactant that reacts the fastest

• The reactant that produces the least product

• The reactant that produces the most product

• The reactant that is left over after the reaction

In the latte example, if you have 4 cups of brewed coffee and 2 cups of milk, how many lattes can you make?

• 1

• 4

• 2

• 6

What is the first step in balancing a chemical equation?

• Add coefficients randomly

• Change the subscripts of the compounds

• Write out all the elements and count them

• Start balancing the elements

When balancing the equation for the reaction between iron(II) chloride and sodium phosphate, what is the coefficient for sodium chloride in the balanced equation?

• 1

• 2

• 3

• 6

What is the purpose of using a mole ratio in stoichiometry?

• To find the molar mass of a compound

• To balance the chemical equation

• To determine the limiting reactant

• To change the compound from reactant to product

If 23 grams of iron(II) chloride reacts with 41 grams of sodium phosphate, which reactant is the limiting reactant?

• Iron(II) chloride

• Sodium phosphate

• Sodium chloride

• Iron(II) phosphate

What is the theoretical yield of sodium chloride if the limiting reactant produces 21 grams of it?

• 41 grams

• 44 grams

• 21 grams

• 16.1 grams

How do you calculate the percent yield of a reaction?

• Add the actual yield to the theoretical yield and divide by 2

• Subtract the actual yield from the theoretical yield

• Divide the theoretical yield by the actual yield and multiply by 100

• Divide the actual yield by the theoretical yield and multiply by 100

If the actual yield of sodium chloride is 16.1 grams and the theoretical yield is 21 grams, what is the percent yield?

• 76.7%

• 80%

• 90%

• 70%

What is the excess reactant in a reaction?

• The reactant that produces the least product

• The reactant that is completely used up

• The reactant that is left over after the reaction

• The reactant that reacts the fastest