Chemical Reactions and Yield Concepts

The video tutorial covers the concept of limiting reagents in chemical reactions, using analogies to explain the process. It details how to convert grams to moles using molar mass, and how to use stoichiometry to find the limiting reagent. The tutorial also explains how to calculate theoretical and actual yields, and how to determine percent yield, considering real-world factors that affect reactions.

What analogy is used to explain the concept of reactants and products?

• Making sandwiches

• Building a house

• Cooking pasta

• Baking a cake

What tool is used in the lab to measure grams of reactants?

• Thermometer

• Balance

• Barometer

• Spectrometer

What is the first step in converting grams of reactants to moles?

• Using stoichiometry

• Using molar mass

• Using a periodic table

• Using a calculator

In the given chemical reaction, which element is the limiting reagent?

• Nitrogen

• Ammonia

• Oxygen

• Hydrogen

How many moles of NH3 are produced from the limiting reagent?

• 10.0 moles

• 7.14 moles

• 5.00 moles

• 12.0 moles

What is the theoretical yield of NH3 in grams?

• 121.4 grams

• 100.0 grams

• 110.0 grams

• 105.7 grams

What term describes the amount of product actually produced in a lab?

• Percent yield

• Actual yield

• Theoretical yield

• Limiting yield

How is percent yield calculated?

• Theoretical yield minus actual yield

• Actual yield plus theoretical yield

• Actual yield divided by theoretical yield times 100%

• Theoretical yield divided by actual yield times 100%

What can cause the actual yield to be less than the theoretical yield?

• Perfect reaction conditions

• Side reactions and incomplete reactions

• Excess reactants

• Accurate measurements

Which term refers to the reactant that is completely consumed first?

• Excess reactant

• Limiting reactant

• Primary reactant

• Secondary reactant