Types of Reactions HW

Al(s) --> Al³⁺ + 3e^-

Zn⁺² + 2 e^- --> Zn

The half-reactions for the oxidation-reduction reaction between Al(s) and Zn²⁺(aq) are represented above. Based on the half-reactions, what is the coefficient for Al(s)

if the equation for the oxidation-reduction reaction is balanced with the smallest whole-number coefficients?

• 1

• 2

• 3

• 4

Tags

NGSS.HS-PS1-7

Ni(s)→Ni²⁺(aq) + 2e⁻

Ag⁺(aq) + e⁻→Ag(s)

Which of the following is the balanced net ionic equation for an oxidation-reduction reaction between Ag⁺(aq) and Ni(s) based on the half-reactions represented above?

• Ag⁺(aq) + Ni(s)→Ag(s) + Ni²⁺(aq)

• 2Ag⁺(aq) + Ni(s)→Ag(s) + 2Ni²⁺(aq)

• Ag⁺(aq) + 2Ni(s)→Ag(s) + 2Ni²⁺(aq)

• 2Ag⁺(aq) + Ni(s)→2Ag(s) + Ni²⁺(aq)

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-7

Cu(s) + 2AgNO₃(aq)→Cu(NO₃)₂(aq) + 2Ag(s)

The reaction between solid copper and aqueous silver nitrate produces solid silver and a blue solution, as represented by the balanced equation shown above. Based on the balanced equation, which of the following identifies the oxidation and reduction half-reactions?

• Oxidation: Cu(s)→Cu⁺(aq) + e⁻

  Reduction: Ag²⁺(aq) + 2e⁻→ Ag(s)

• Oxidation: Cu(s)→Cu⁺²(aq) + 2e⁻

  Reduction: Ag⁺(aq) + e⁻→ Ag(s)

• Oxidation: Ag⁺(aq) + e⁻→ Ag(s)

  Reduction: Cu(s)→Cu⁺²(aq) + 2e⁻

• Oxidation: Ag²⁺(aq) + 2e⁻→ Ag(s)

  Reduction: Cu(s)→Cu⁺(aq) + e⁻

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-7

The diagrams above represent solutes present in two different dilute aqueous solutions before they were mixed. Water molecules are not shown. When the solutions were combined, a precipitation reaction took place. Which of the diagrams below is the best particle representation of the mixture after the precipitation reaction occurred?

• 
• 
• 
• 

Tags

NGSS.HS-PS1-7

When C₂H₄(g) reacts with H₂(g), the compound C₂H₆(g)

is produced, as represented by the equation above. The reaction is correctly classified as which of the following types?

• Acid-base, because two hydrogen atoms are donated to C₂H₄ (g)

  .

• Precipitation, because two reactant species form a single product.

• Decomposition, because pure H₂(g) is consumed.

• Oxidation-reduction, because H₂(g) is oxidized.

I₂(aq) + C₆H₈O₆(aq)→C₆H₆O₆(aq) + 2I⁻(aq) + 2H⁺(aq)

The compound C₆H₈O₆ reacts with I₂ according to the reaction represented by the equation above. The reaction is correctly classified as which of the following types?

• Acid-base, because H⁺ ions are produced.

• Precipitation, because there are only two reactants but there are three products.

• Double replacement, because both H and I appear as ions in the products.

• Oxidation-reduction, because I₂ is reduced.

Cu(s) + 4 HNO₃(aq) → Cu(NO₃)₂(aq) + 2 NO₂(g) + 2 H₂O(l)

Each student in a class placed a 2.00g sample of a mixture of Cu and Al in a beaker and placed in a beaker and placed the beaker in a fume hood. The students slowly poured 15.0 mL of 15.8 M HNO₃(aq) into their beakers. The reaction between the copper in the mixture and the HNO₃(aq) is represented by the equation above. The student observed that a brown gas was released from the beakers and that the solutions turned blue, indicating the formation of Cu²⁺(aq). The solutions were then diluted with distilled water to known volumes.

Which of the following is true about this reaction?

• It is a Brønsted-Lowry acid-base reaction, because the solution is neutral at the end.

• It is a Brønsted-Lowry acid-base reaction, because HNO₃(aq) is a strong acid.

• It is a redox reaction, because Cu(s) is oxidized and H⁺(aq) is reduced.

• It is a redox reaction, because Cu(s) is oxidized and the nitrogen atom in NO₃⁻(aq) is reduced.

Tags

NGSS.HS-PS1-2

Which of the following is the conjugate acid of NH₂^- ?

• NH^2-

• NH₃

• H⁺

• NH₄⁺