Limiting reagents

The limiting reactant

• slows the reaction down
• is used up first
• is the reactant that is left over
• controls the speed of the reaction

Theoretical yield = 73g

Actual yield = 62g

Calculate the percent yield.

• 116%

• 85%

• 1.16%

• 76%

Tags

NGSS.HS-PS1-7

3. The reactant that is not completely used up in a chemical reaction is called the __________ .

• spectator reagent
• limiting reagent
• excess reagent
• catalyst

Tags

NGSS.HS-PS1-7

4. If the quantities of reactants are given in units other than moles, what is the first step for determining the amount of product?

• Determine the amount of product from the given amount of limiting reagent.
• Convert each given quantity of reactant to moles.
• Identify the limiting reagent.

Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl₂.

Mg + 2HCl --> MgCl₂ + H₂

• Mg

• H₂

• MgCl₂

• HCl

Tags

NGSS.HS-PS1-7

When you use a balanced chemical equation to calculate the amount of a product on paper it is referred to as the 

• experimental value
• theoretical value
• true amount
• percent yield

Tags

NGSS.HS-PS1-7

A reaction was predicted to produce 32.4 grams of a compound. When the product was measured, there were only 26.1 grams made. What is the percent yield?

• 80.6%
• 6.3%
• 24.1%
• 58.5%

Tags

NGSS.HS-PS1-7

1 Cheese + 2 Bread --> 1 Grilled cheese
How many grilled cheeses can you make with 26 slices of bread and 14 pieces of cheese?

• 14
• 13
• 26
• 7

Cl₂ + 2 KBr → Br₂ + 2 KCl

How many grams of potassium chloride can be produced from 356 g of Cl₂ and 356 g of potassium bromide?

• 749 g

• 223 g

• 479 g

• 814 g

4NH₃ + 5O₂ --> 4NO + 6H₂O

The amount of NO formed using 6.30g of NH₃ is 11.1 g NO. The amount of NO formed using 1.80g of O₂ is 1.35 g NO. Determine the amount of excess reagent that is not used up during the reaction.

• 0.765g

• 5.54g

• 1.35g

• 11.1g