Question 1

The ________ is the amount of product that forms when all the limiting reactant reacts to form the desired product.

Accepted Answer

The answer of The ________ is the amount of product...

Question 2

How many grams of magnesium oxide remain after 18.50 g of magnesium oxide reacts with 30.30 g hydrochloric acid to produce magnesium chloride and water?

Accepted Answer

The answer of How many grams of magnesium oxide remain...

Question 3

The ________ is the amount of product physically collected from a chemical reaction and is typically less than the theoretical yield.

Accepted Answer

The answer of The ________ is the amount of product...

Question 4

________ is defined by the following equation
  × 100%

Accepted Answer

The answer of ________ is defined by the following equation
...

Question 5

The molecular formula is a whole number multiple of the empirical formula.

Accepted Answer

This is a rule in chemistry known as the law of multiple proportions. The molecular formula represents the actual number of atoms in a molecule, while the empirical formula represents the simplest ratio of the atoms in the molecule. Since the molecular formula must have a whole number multiple of the empirical formula, the law of multiple proportions is always followed. This is true. The molecular formula represents the actual number of atoms of each element in a molecule, while the empirical formula gives the simplest whole-number ratio of the atoms in a molecule. Since the molecular formula represents a multiple of the empirical formula, the molecular formula will always be a whole number multiple of the empirical formula.

Question 6

What is the theoretical yield of calcium oxide, in grams, that can be produced by the reaction of 5.61 g of V₂O₅ with 7.44 g of calcium to produce vanadium and calcium oxide? (Show all your work)

Accepted Answer

The answer of What is the theoretical yield of calcium...

Question 7

Ammonia reacts with oxygen to form nitrogen monoxide and water. What is the theoretical yield and the percent yield if 17.25 g of nitrogen monoxide is produced when 21.50 g of ammonia and 26.85 g of oxygen react? (Show all your work)

Accepted Answer

The answer of Ammonia reacts with oxygen to form nitrogen...

Question 8

What is the coefficient of H₂O when the following equation is properly balanced with the smallest set of whole numbers? ________ Na + ________ H₂O → ________ NaOH + ________ H₂

Accepted Answer

The answer of What is the coefficient of H₂O when...

Question 9

Many compounds can be represented with the same empirical formula.

Accepted Answer

This is true. Empirical formulas represent the simplest ratio of elements in a compound, so compounds with different molecular formulas can have the same empirical formula if they have the same relative number of atoms. This is true, as empirical formulas only give the simplest ratio of atoms in a compound and do not specify the actual arrangement of atoms or the molecular formula. Therefore, different compounds with different structures can have the same empirical formula. For example, both methane (CH4) and ethene (C2H4) have the same empirical formula, CH4.

Question 10

The insecticide DDT was formerly in widespread use, but now it is severely restricted owing to its adverse environmental effects. It is prepared as follows: C₂HCl₃O + C₆H₅Cl → C₁₄H₉Cl₅+H₂O [unbalanced] chloral chlorobenzene DDT Suppose 10.00 g of chloral was put in a container with 10.00 g of chlorobenzene and allowed to react. a. What is the maximum amount, in mol, of DDT which could be formed? b. What is the limiting reactant? c. What is the percent yield, if 12.15 g of DDT is produced?

Accepted Answer

The answer of The insecticide DDT was formerly in widespread...

Question 11

There is only one distinct empirical formula for each compound that exists.

Accepted Answer

The empirical formula is the simplest whole number ratio of the elements in a compound. Therefore, each compound can have only one distinct empirical formula. However, different compounds can have the same empirical formula if they have the same ratio of elements. The empirical formula represents the simplest whole number ratio of atoms present in a compound. Therefore, each compound can have only one distinct empirical formula. However, compounds may have the same empirical formula but different molecular formulas.

Question 12

The ________ is defined by the following equation:
  × 100%

Accepted Answer

The answer of The ________ is defined by the following...

Question 13

The limiting reactant is the reactant with the smallest initial mass.

Accepted Answer

The limiting reactant is the reactant that is completely consumed in a chemical reaction, thus limiting the amount of product that can be formed. The limiting reactant can only be determined by comparing the mole ratios of the reactants, not their initial masses.

Question 14

The percent yield can be determined by dividing the actual yield by the theoretical yield and multiplying this value by 100%.

Accepted Answer

This is the correct formula for calculating percent yield.

Question 15

What is the coefficient of O₂ when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? ________ C₁₈H₃₆O₂ + ________ O₂→ ________ CO₂ + ________ H₂ O

Accepted Answer

The answer of What is the coefficient of O₂ when...

Question 16

The empirical formula is the simplest whole number ratio of atoms representing a chemical formula of a molecule.

Accepted Answer

This is true. The empirical formula is a representation of the simplest ratio of atoms in a compound. It does not necessarily represent the actual molecular formula. The definition of empirical formula is correct and represents the true nature of the concept.

Question 17

The ________ is the one component that is completely consumed during a chemical reaction.

Accepted Answer

The answer of The ________ is the one component that...

Quiz 3: Stoichiometry: Ratios of Combination

The ________ is the amount of product that forms when all the limiting reactant reacts to form the desired product.

How many grams of magnesium oxide remain after 18.50 g of magnesium oxide reacts with 30.30 g hydrochloric acid to produce magnesium chloride and water?

The ________ is the amount of product physically collected from a chemical reaction and is typically less than the theoretical yield.

________ is defined by the following equation × 100%

The molecular formula is a whole number multiple of the empirical formula.

What is the theoretical yield of calcium oxide, in grams, that can be produced by the reaction of 5.61 g of V₂O₅ with 7.44 g of calcium to produce vanadium and calcium oxide? (Show all your work)

Ammonia reacts with oxygen to form nitrogen monoxide and water. What is the theoretical yield and the percent yield if 17.25 g of nitrogen monoxide is produced when 21.50 g of ammonia and 26.85 g of oxygen react? (Show all your work)

What is the coefficient of H₂O when the following equation is properly balanced with the smallest set of whole numbers? Na + H₂O → NaOH + H₂

Many compounds can be represented with the same empirical formula.

There is only one distinct empirical formula for each compound that exists.

The ________ is defined by the following equation: × 100%

The limiting reactant is the reactant with the smallest initial mass.

The percent yield can be determined by dividing the actual yield by the theoretical yield and multiplying this value by 100%.

What is the coefficient of O₂ when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? C₁₈H₃₆O₂ + O₂→ CO₂ + H₂ O

The empirical formula is the simplest whole number ratio of atoms representing a chemical formula of a molecule.

The ________ is the one component that is completely consumed during a chemical reaction.

Quiz 3: Stoichiometry: Ratios of Combination

The ________ is the amount of product that forms when all the limiting reactant reacts to form the desired product.

How many grams of magnesium oxide remain after 18.50 g of magnesium oxide reacts with 30.30 g hydrochloric acid to produce magnesium chloride and water?

The ________ is the amount of product physically collected from a chemical reaction and is typically less than the theoretical yield.

________ is defined by the following equation × 100%

The molecular formula is a whole number multiple of the empirical formula.

What is the theoretical yield of calcium oxide, in grams, that can be produced by the reaction of 5.61 g of V2O5 with 7.44 g of calcium to produce vanadium and calcium oxide? (Show all your work)

Ammonia reacts with oxygen to form nitrogen monoxide and water. What is the theoretical yield and the percent yield if 17.25 g of nitrogen monoxide is produced when 21.50 g of ammonia and 26.85 g of oxygen react? (Show all your work)

What is the coefficient of H2O when the following equation is properly balanced with the smallest set of whole numbers? ________ Na + ________ H2O → ________ NaOH + ________ H2

Many compounds can be represented with the same empirical formula.

There is only one distinct empirical formula for each compound that exists.

The ________ is defined by the following equation: × 100%

The limiting reactant is the reactant with the smallest initial mass.

The percent yield can be determined by dividing the actual yield by the theoretical yield and multiplying this value by 100%.

What is the coefficient of O2 when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? ________ C18H36O2 + ________ O2 → ________ CO2 + ________ H2 O

The empirical formula is the simplest whole number ratio of atoms representing a chemical formula of a molecule.

The ________ is the one component that is completely consumed during a chemical reaction.

What is the theoretical yield of calcium oxide, in grams, that can be produced by the reaction of 5.61 g of V₂O₅ with 7.44 g of calcium to produce vanadium and calcium oxide? (Show all your work)

What is the coefficient of H₂O when the following equation is properly balanced with the smallest set of whole numbers? Na + H₂O → NaOH + H₂

What is the coefficient of O₂ when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? C₁₈H₃₆O₂ + O₂→ CO₂ + H₂ O