In this reaction Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) Magnesium acts as a reducing agent.
Explanation
Magnesium metal is being oxidized to magnesium cations, Mg2+. Hydrogen is being reduced from hydrogen ions, H+, to hydrogen gas, H2. So we can conclude that the above reaction is a redox reaction. Therefore, you can say that magnesium is acting as a reducing agent because it reduces hydrogen to hydrogen gas while being oxidized in the process. In contrast, hydrochloric acid plays an oxidising agent’s role as it oxidizes magnesium to magnesium cations while being reduced in the process.
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This is an oxidation-reduction (redox) reaction:
2 HI+2 e-→2 H0(reduction)
Mg0 -2 e-→MgII(oxidation)
HCl is an oxidizing agent, Mg is a reducing agent.
Reactants:
- Mg
- Names: Magnesium , Magnesium (powder), Magnesium (pellets)
- Appearance: Grey powder
; Silvery-white metallic solid in various forms
- Names: Magnesium
- HCl – Chlorane
, Hydrogen chloride
- Other
names: Hydrochloric acid
, M, Uriatic acid
- Appearance: Colorless, transparent liquid, fumes in air if concentrated
; Colorless gas; Colourless compressed liquefied gas with pungent odour; Colorless to slightly yellow gas with a pungent, irritating odor. [Note: Shipped as a liquefied compressed gas.]
- Other
names: Hydrochloric acid
Products:
- H2
- Names: Dihydrogen
, Hydrogen, H2
- Appearance: Odourless colourless compressed gas
- Names: Dihydrogen
- MgCl2
- Names: Magnesium chloride
, Magnesium dichloride, Magnesium chloride anhydrous
- Appearance: White or colourless crystalline solid
; Deliquescent white solid in various forms
- Names: Magnesium chloride