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Oxidation-Reduction (Redox) Calculator

LivePhysics

Electron Transfer Diagram

ZnOxidizedCuReduced2e⁻Loses electrons → Gains electronsReducing agent: ZnOxidizing agent: CuSO4

Reaction

Results

Zn oxidation change
0 → +2 (oxidized)
Cu oxidation change
+2 → 0 (reduced)
Oxidized (loses electrons)
Zn
Reduced (gains electrons)
Cu
Reducing Agent
Zn
Oxidizing Agent
CuSO4
Electrons Transferred
2

Step-by-Step

1. Assign oxidation numbers (reactants)

Zn: Zn: 0CuSO4: O: −2,  S: +6,  Cu: +2\text{Zn: }\text{Zn: }0 \quad \text{CuSO4: }\text{O: }-2, \;\text{S: }+6, \;\text{Cu: }+2

2. Assign oxidation numbers (products)

ZnSO4: O: −2,  S: +6,  Zn: +2Cu: Cu: 0\text{ZnSO4: }\text{O: }-2, \;\text{S: }+6, \;\text{Zn: }+2 \quad \text{Cu: }\text{Cu: }0

3. Identify oxidation number changes

Zn: 0→+2  (oxidized)Cu: +2→0  (reduced)\text{Zn: }0 \to +2\;(\text{oxidized}) \quad \text{Cu: }+2 \to 0\;(\text{reduced})

4. Electron transfer

Zn loses 2 electrons (oxidized), Cu gains 2 electrons (reduced)\text{Zn loses 2 electrons (oxidized), Cu gains 2 electrons (reduced)}

5. Identify agents

Oxidizing agent: CuSO4, Reducing agent: Zn\text{Oxidizing agent: CuSO4, Reducing agent: Zn}

Reference Guide

Free redox reaction analyzer. Enter a chemical reaction to identify oxidation state changes, electron transfers, and oxidizing and reducing agents with step-by-step KaTeX.

Oxidation Numbers

primary

Oxidation and Reduction

secondary

Agents

tertiary

Balancing Redox