Given the unbalanced equation, for the species that is the reduction product, en

Question

Given the unbalanced equation, for the species that is the reduction product, enter the symbol and the final oxidation state of the specific element that has a lower oxidation state. Use arabic numerals for oxidation state magnitude.

Example:

Element: Sb

Oxidation state: 0

Zn(s) + Au3+(aq) + Cl-(aq) ? Au(s) + Zn2+(aq) + Cl-(aq)

Given the unbalanced equation, for the species that is the reduction product, enter the symbol and the final oxidation state of the specific element that has a lower oxidation state. Use arabic numerals for oxidation state magnitude. Example: Element: Sb Oxidation state: 0 Zn(s) + Au3+(aq) + Cl-(aq) ? Au(s) + Zn2+(aq) + Cl-(aq) Element: Oxidation state:

Explanation / Answer

Zn(s) + Au3+(aq) + Cl-(aq) ? Au(s) + Zn2+(aq) + Cl-(aq)

1)Zn ------Zn2+

Zn changes from 0 to +2 oxidation state

here Zn is oxidised

2) Au3+(aq) -----> Au(s)

Al changes from +3 to 0 oxidation state

here Al is reduced.

3) Cl-(aq) -----> Cl-(aq)

Cl changes from -1 to -1 oxidation state

=> there is no change

=> it will neither oxidised nor reduced

Related Questions

Navigate

• Browse (All)
• Browse G
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.