Actual Yield

The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting

• Percent
• actual
• stoichiometry
• theoretical

Tags

112.43.c.9.C

When reacting Na with Cl₂, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

• 90.4%

• 104%

• 96.15%

• 1.04%

Tags

112.43.c.9.C

Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.

• 1.16%
• 116%
• 85%
• 76%

Tags

112.43.c.9.C

In a lab, a scientist calculate 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%
• 0.82%
• 10.1 %
• 100%

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112.43.c.9.C

Reactant and products might adhere to containers causing actual yield to be less than theoretical yield.

• true

• false

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112.43.c.9.C

Competing reactions might occur forming other products causing your actual yield to be less than your theoretical yield.

• true

• false

Tags

112.43.c.9.C

Some product may be lost during filtering causing your actual yield to be less than your theoretical yield.

• true

• false

Tags

112.43.c.9.C

What is the equation to calculate percent yield?

• (Actual yield / Theoretical yield) x 100% = Percent yield

• (Theoretical yield / Actual yield) x 100% = Percent yield

• Mass (1 Mole / Molar mass) x 100% = Percent yield

• Mass x Speed x 100% = Percent yield

Tags

112.43.c.9.C

What does percent yield indicate?

• The mass of product that should be obtained

• How quickly the reaction is completed

• The product of product actually obtained

• The efficiency of the chemical reaction

Tags

112.43.c.9.C

Which of the following is NOT a reason for the actual yield to be different from the theoretical yield?

• some product is lost in purification

• more excess reactant is added

• competing reactions may use up reactants

• the limiting reactant may not be 100% pure

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112.43.c.9.C