11.4 % Yield

What is the maximum amount of product that can be produced from a given amount of reactant?

• percent yield

• theoretical yield

• actual yield

• mole ratio

Tags

NGSS.HS-PS1-7

The reaction of 5.0 grams of fluorine with excess chlorine produced 5.6 grams of ClF₃. What percent yield of ClF₃ was obtained?

Cl₂ + 3F₂ → 2ClF₃

• 58%

• 69%

• 76%

• 86%

In the bunsen burner reaction of methane and oxygen, what is the percent yield if 64.0 g of methane yields 95.1 grams of carbon dioxide?

CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g)

• 46 %

• 54%

• 149%

• 50%

Percent yield should never be greater than ________.

• theoretical yield

• 100%

• both a and b

• 50%

The statement that percent yield can never be greater than theoretical yield is another example of the ________.

• ideal gas law

• law of conservation of mass

• law of conservation of momentum

• law of conservation of energy

Theoretical yield = 73 g

Actual yield = 62 g

Calculate the percent yield.

• 1.16 %

• 116 %

• 85 %

• 76 %

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

• theoretical yield
• mole ratio
• actual yield
• percentage yield

Tags

NGSS.HS-PS1-7

P₄ + 6Cl₂ → 4PCl₃

The reaction of 75 g P₄ with excess chlorine gas produces 110 g PCl₃ in lab. Calculate percent yield for the reaction.

• 78%

• 64%

• 27%

• 33%

Be + 2HCl → BeCl₂ + H₂

My theoretical yield of beryllium chloride was 10.7 grams. If my actual yield was 4.5 grams, what was my percent yield?

• 42 %

• 2.4 %

• 1.2 %

• 27 %

Tags

NGSS.HS-PS1-7

4NH₃ + 5O₂ --> 4NO + 6H₂O

If 1.21 g of NO are formed when 6.30 g of ammonia react with 1.80 g of oxygen, what is the % yield?

• 37.0 %

• 45.1 %

• 89.6%

• 10.9 %