Theoretical Yield & Losses

The video tutorial explains the concept of theoretical yield in chemical reactions, which is the maximum possible amount of product that can be produced. It provides a step-by-step guide on calculating theoretical yield using magnesium chloride as an example. The tutorial also discusses practical considerations and reasons why the theoretical yield is often not achieved in real-world scenarios, such as incomplete reactions, purification losses, and equilibrium states. The video concludes with a summary of these key points.

What is the theoretical yield in a chemical reaction?

• The actual amount of product obtained

• The maximum possible amount of product that can be produced

• The amount of reactants used

• The minimum amount of product required

How do you calculate the formula mass of magnesium chloride?

• Add the atomic mass of magnesium to the atomic mass of one chlorine atom

• Multiply the atomic mass of magnesium by two

• Add the atomic mass of magnesium to the atomic mass of two chlorine atoms

• Subtract the atomic mass of chlorine from magnesium

If you start with 12.15 grams of magnesium, what is the theoretical yield of magnesium chloride?

• 12.15 grams

• 95.3 grams

• 24.3 grams

• 47.65 grams

Which of the following is NOT a reason for not achieving the theoretical yield?

• Incomplete reactions

• Loss of product during purification

• Alternative reactions producing different products

• All reactants converting to desired product

What happens when a reaction is in equilibrium?

• The products can revert back to reactants

• The reaction stops completely

• The reaction only moves forward

• All reactants are converted to products