Chemistry Ch7: Quizzes

Which chemical equation correctly represents the reaction of one methane (CH₄) molecule reacting with oxygen (O₂) to form carbon dioxide (CO₂) and water (H₂O)?

 

A. CH₄ + 2O₂ → CO₂ + 2H₂O

B. CH₄ + O₂ → CO₂ + H₂O

C. 2CH₄ + O₂ → 2CO₂ + H₂O

D. CH₄ + O₂ → CO₂ + 2H₂O

A

What do coefficients in a chemical equation show?

 

A. The names of the substances

B. The relative amounts of reactants and products

C. The charges of atoms

D.The color of the substances

B

Balance the equation

H₂ + O₂ ⟶ H₂O

 

A. H₂ + O₂ ⟶ H₂O
B. 2H₂ + O₂ ⟶ 2H₂O
C. H₂ + 2O₂ ⟶ 2H₂O
D. 2H₂ + 2O₂ ⟶ H₂O

B

Balance the equation

Al + O₂ ⟶ Al₂O₃

A. Al + O₂ ⟶ Al₂O₃
B. 2Al + O₂ ⟶ Al₂O₃
C. 4Al + 3O₂ ⟶ 2Al₂O₃
D. 2Al + 3O₂ ⟶ Al₂O₃

C

For the Combustion of propane

C₃H₈ + O₂ ⟶ CO₂ + H₂O

Which is the correctly balanced equation?

A. C₃H₈ + 4O₂ ⟶ 3CO₂ + 4H₂O
B. C₃H₈ + 5O₂ ⟶ 3CO₂ + 4H₂O
C. 2C₃H₈ + 5O₂ ⟶ 6CO₂ + 8H₂O
D. C₃H₈ + 3O₂ ⟶ 3CO₂ + 4H₂O

B

Which of the following correctly matches the physical state abbreviation to its meaning in a chemical equation?

A. (s) = gas, (l) = liquid, (g) = solid, (aq) = dissolved in water
B. (s) = solid, (l) = liquid, (g) = gas, (aq) = dissolved in water
C. (s) = solid, (l) = gas, (g) = liquid, (aq) = solid in water
D. (s) = solution, (l) = liquid, (g) = gas, (aq) = gas in water

B

Which of the following statements correctly explains why a precipitation reaction occurs when AgNO₃ and NaCl solutions are mixed?

A) All cations react with all anions to form insoluble compounds.
B) Only the pairing of Ag⁺ and Cl⁻ forms an insoluble salt, while the other combinations remain soluble.
C) Nitrate ions (NO₃⁻) form insoluble salts with sodium ions (Na⁺).
D) Sodium chloride is insoluble in water, causing it to precipitate.

B

Which solution could be used to precipitate the silver ion (Ag⁺) from a water sample, and what is the formula of the expected precipitate?

A. Sodium chloride, NaCl → AgCl (s)
B. Sodium nitrate, NaNO₃ → AgNO₃ (aq)
C. Sodium hydroxide, NaOH → AgOH (aq)
D. Sodium sulfate, Na₂SO₄ → Ag₂SO₄ (aq)

A

Which solution could be used to precipitate the calcium ion (Ca²⁺) from a water sample, and what is the formula of the expected precipitate?

A. Sodium carbonate, Na₂CO₃ → CaCO₃ (s)
B. Sodium hydroxide, NaOH → Ca(OH)₂ (aq)
C. Sodium sulfate, Na₂SO₄ → CaSO₄ (s)
D. Both A and C

D

In aqueous solutions, an acid is defined as a substance that:

 

A. Produces hydroxide ions (OH⁻) when dissolved in water 

B. Produces hydrogen gas (H₂) when dissolved in water

C. Produces hydronium ions (H₃O⁺) when dissolved in water 

D. Reacts only with metals

C

Why do we write a net ionic equation instead of the full molecular equation?

 

A. To include all ions present in solution 

B. To balance charges only

C. To show only the species that actually change during the reaction

D. To predict the color of the solution

C

What is the net ionic equation for the reaction between H₂SO₄ (strong acid) and LiOH (strong base)?

A) H₂SO₄ + 2LiOH → Li₂SO₄ + 2H₂O
B) H⁺ + OH⁻ → H₂O
C) Li⁺ + SO₄²⁻ → Li₂SO₄
D) H₂SO₄ + LiOH → LiHSO₄ + H₂O

B

How many moles of NaOH are required to completely react with 0.75 mol of H₂SO₄ according to the equation:

H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O

1.50 mol

The reaction of hydrogen and chlorine is represented by the balanced equation:

H₂ + Cl₂ → 2HCl

If 3 moles of H₂ are combined with 2 moles of Cl₂, which statement is correct?
 

A. Hydrogen is in excess, chlorine is limiting, and all hydrogen reacts.

B. Hydrogen is the limiting reactant, chlorine is in excess, and 1 mol of Cl₂ remains unreacted.

C. Hydrogen and chlorine are present in the exact stoichiometric ratio, so none remains unreacted.

D. Chlorine is the limiting reactant, hydrogen is in excess, and 1 mol of H₂ remains unreacted.

D

ionic compound that can be formed by the reaction of an acid with a base that contains a cation and an anion other than hydroxide or

salt

substance added to the sample in a titration analysis to permit visual detection of the end point

indicator

number placed in front of symbols or formulas in a chemical equation to indicate their relative amount

coefficient

reaction involving the transfer of a hydrogen ion between reactant species

acid-base reaction

reactant present in an amount lower than required by the reaction stoichiometry, thus limiting the amount of product generated

limiting reactant

relationships between the amounts of reactants and products of a chemical reaction

stoichiometry