Which of the following is NOT a reason why the actual yield of a reaction is less than the theoretical yield?

The reaction is reversible and does not go to completion.
Some products are lost during separation from the reaction mixture.
All reactants react exactly as expected.
Some reactants may react in unexpected ways.

Use some of the following answers to fill in the blanks:
Reversible, incomplete, exothermic, irreversible

Even though no atoms are lost or gained in a chemical reaction, the actual yield may be less than the theoretical yield because the reaction may not go to completion as it is .

Select all the reasons why the actual yield may be less than the theoretical yield.

The reaction is reversible.
Products are lost during separation.
Reactants form unexpected products.
The reaction is exothermic.

What is the formula to calculate the percentage yield of a product?

(Actual yield / Theoretical yield) × 100
(Theoretical yield / Actual yield) × 100
(Actual yield × Theoretical yield) × 100
(Actual yield – Theoretical yield) × 100

Calculate the percentage yield of a reaction where the theoretical yield is 50 grams and the actual yield is 40 grams.

The percentage yield is .

Magnesium reacts with hydrochloric acid to produce magnesium chloride and hydrogen gas according to the equation:

Mg + 2HCl → MgCl₂ + H₂

Calculate the theoretical mass of magnesium chloride if 24 grams of magnesium are used.
Mg Ar = 24
MgCl₂ Mr = 95

g

Match each term to its correct definition.

Ratio of actual yield to theoretical yield expressed as a percentage
Maximum amount of product that could be formed from given reactants

Percentage yield
Theoretical yield

Why is a high atom economy important in chemical manufacturing?

It reduces waste and is more sustainable.
It increases the amount of by-products.
It decreases the cost of reactants.
It allows for faster reactions.

Use some of the following answers to fill in the blanks:
Desired, by-products, reactants, unwanted, additional

Atom economy = (Relative formula mass of product / Sum of relative formula masses of all ) × 100

[question number = 05.5] Calculate the atom economy for the production of ethanol in the fermentation of glucose:

C₆H₁₂O₆ → 2C₂H₅OH + 2CO₂

Relative formula masses: C₆H₁₂O₆=180, C₂H₅OH=46, CO₂=44

Give your answer to 1 decimal place.

The atom economy is .

Select all the factors that are considered when choosing a reaction pathway to produce a specific product.

Atom economy
Yield
Rate of reaction
Equilibrium position
Usefulness of by-products

Which of the following statements about atom economy is TRUE?

A reaction with high atom economy produces less waste.
Atom economy does not affect sustainability.
High atom economy reactions are always faster.
Atom economy is unrelated to useful product amount.

Use some of the following answers to fill in the blanks:
Speed, volume, concentration, moles, area

The concentration of a solution in mol/dm³ is equal to the amount in of solute divided by the in dm³.

A solution contains 0.5 moles of sodium chloride in 250 cm³ of solution. Calculate its concentration in mol/dm³.

mol/dm³

If the volumes of two solutions that react completely are known and the concentration of one solution is known, what can be calculated?

The concentration of the other solution.
The mass of the reactants.
The theoretical yield.
The pressure of the system.

At room temperature and pressure, one mole of any gas occupies a volume of:

22.4 dm³
24 dm³
20 dm³
12 dm³

Calculate the volume of 88 grams of carbon dioxide gas at room temperature and pressure.
Relative atomic masses: C=12, O=16)

dm³

Which of the following is the correct formula to calculate the volume of a gas at room temperature and pressure?

Volume = Moles × 24 dm³/mol
Volume = Moles × 22.4 dm³/mol
Volume = Moles × 12 dm³/mol
Volume = Moles × 44 dm³/mol

Yield, Atom Economy, Concentrations and Gas Volumes Quiz

Good Luck!

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