Limiting Reactants and Percent Yield

If a chemist calculates the maximum amount of product that could be obtained from a chemical reaction, he or she is calculating the

• Theoretical yield

• Mole ratio

• Actual yield

• Percentage yield

Tags

NGSS.HS-PS1-7

Cl₂ + 2KBr → Br₂ + 2KCl

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

• 749 g

• 223 g

• 479 g

• 814 g

Tags

NGSS.HS-PS1-7

What is the measured amount of a product obtained from a chemical reaction?

• Mole ratio

• Theoretical yield

• Percentage yield

• Actual yield

Tags

NGSS.HS-PS1-7

Mg + 2HCl → MgCl₂ + H₂

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

• Mg

• H₂

• MgCl₂

• HCl

In a lab, a scientist calculated that he should produce 12.3 grams of product in his experiment. When he is finished collecting his product, it weighs 10.1 grams. What is his percent yield?

• 82.1%

• 0.82%

• 10.1%

• 122%

Tags

NGSS.HS-PS1-7

4NH₃ + 6NO → 5N₂ + 6H₂O

What is the limiting reactant if 10 moles of NH₃ react with 30 moles of NO?

• NH₃

• NO

• N₂

• H₂O

Tags

NGSS.HS-PS1-7

A chemist interested in the efficiency of a chemical reaction would calculate the

• Mole ratio

• Rate of reaction

• Percent yield

• Energy released

Tags

NGSS.HS-PS1-5

4NH₃ + 5O₂ → 4NO + 6H₂O

How many grams of NO are formed if 6.30 g of ammonia react with 1.80 g of oxygen?

• 0.370 g

• 0.0450 g

• 1.35 g

• 11.1 g

Tags

NGSS.HS-PS1-7

What is an excess reactant?

• Substance you end with

• Substance that determines the rate of reaction

• Substance that is not used up completely

• Substance that is used up completely

CH₄ + 2H₂O → CO₂ + 4H₂

How many grams of CO₂ will form when 20.0 g of CH₄ reacts with 15.0 g of H₂O?

• 65.3 g

• 18.3 g

• 54.8 g

• 15.0 g

Tags

NGSS.HS-PS1-7