Question

Determine the oxidizing agent, reducing agent, the substance being oxidized, and the substance being reduced in each reaction in Part 1. Write the reduction half reactions for all four reactions in Part 1.

It was put into a solution of copper gluconate with dH2O and NaCl  

Metal | Al (Trial 1) 2.5 g Al (Trial 2) Zn (Trial 1) Filter Paper Mass (9) Filter paper + Cu Mass (g) Cu Mass (g) Avg. Cu Mass (g) 2.3 g 2.9 g 0.6 g 0.4 g 2.3 g 0.2 g 2.3 g 0.25 g 2.3 g 2.5 g 0.2 g 2.6 g 0.4 g 2.6 g 0.3 g Zn (Trial 2) coco Fe (Trial 1) 2.3 g 0.3 g Fe (Trial 2) 2.3 g 2.8 g 0.5 g caca Sn (Trial 1) 2.3 g 2.8 g 0.5 g 0.4 g Sn (Trial 2) 2.3 g 2.6 g 0.3 g

Answer 1

oxidizing agent: The species reduces itself (gains electrons) and oxidises other .

reducing agent : The species oxidises itself (loses electron ) and reduces other.

1.

2 Al + 3Cu²⁺ $\rightarrow$   2Al³⁺ + 3 Cu

Oxidation reaction : Al - 3e  $\rightarrow$ Al³⁺

Reduction reaction : Cu²⁺ + 2e  $\rightarrow$ Cu

Hence Al is oxidized and Cu²⁺ is reduced.

Al is reducing agent and Cu²⁺ ( copper gluconate ) is oxidizing agent.

2.

Zn is oxidized

Oxidation reaction: Zn - 2e $\rightarrow$ Zn²⁺.

Cu²⁺ is reduced.

Reduction reaction : Cu²⁺ +2e $\rightarrow$ Cu

Zn is reducing agent and Cu²⁺ is oxidising agent.

3.

Fe+ Cu²⁺$\rightarrow$ Fe²⁺ + Cu

Oxidation reaction : Fe - 2e $\rightarrow$ Fe²⁺

reduction reaction : Cu²⁺ + 2e $\rightarrow$ Cu

Fe is oxidized and Cu²⁺ is reduced.

Fe is reducing agent and Cu²⁺ is oxidizing agent.

4.

Sn + Cu²⁺$\rightarrow$ Sn²⁺ + Cu

Oxidation reaction : Sn - 2e $\rightarrow$ Sn²⁺

Reduction reaction : Cu²⁺ - 2e $\rightarrow$ Cu

Sn is oxidized and Cu²⁺ is reduced.

Sn is reducing agent and Cu²⁺ is oxidizing agent.