Chromate-Dichromate Equilibrium

2CrO42− + 2H+ ⇌ Cr2O72− + H2O

개요

Chromate (yellow, CrO₄²⁻) converts to dichromate (orange, Cr₂O₇²⁻) in acidic solution and vice versa in basic solution. This pH-dependent equilibrium involves condensation of two tetrahedral chromate units. While chromium remains at +6 throughout, this equilibrium is fundamental to Cr(VI) redox chemistry.

참여 물질

역할 물질 계수 상태
생성물 Water H₂O 1 (l)

일상 속 예시

Adding acid to yellow potassium chromate solution turns it orange, and adding base reverses it, demonstrating Le Chatelier's principle.

산업적 중요성

크롬산/이크롬산 평형은 크롬 도금, 가죽 무두질, 그리고 Cr(VI) 환경 오염의 이해에 중요합니다.

성질

유형
Redox
가역 반응
예
에너지
발열
ΔH
-14.0 kJ/mol

관련 반응

Iron(II) to Iron(III) Oxidation by Oxygen Bleaching with Sodium Hypochlorite Copper Reduction of Silver Ion Aqua Regia Dissolving Gold Cerium(IV) Reduction by Iron(II) Chlorine Oxidation of Bromide Copper Oxidation by Nitric Acid Hypochlorite Oxidation of Hydrogen Peroxide Hydrogen Peroxide as Oxidizing Agent (Acidic) Displacement of Hydrogen from Acid by Magnesium

Frequently Asked Questions

What is the equation for Chromate-Dichromate Equilibrium?
The balanced equation is: 2CrO₄²⁻ + 2H⁺ ⇌ Cr₂O₇²⁻ + H₂O.
What type of reaction is Chromate-Dichromate Equilibrium?
Chromate-Dichromate Equilibrium is a redox reaction. It is reversible under certain conditions.
Is Chromate-Dichromate Equilibrium exothermic or endothermic?
Chromate-Dichromate Equilibrium is exothermic (releases energy). The enthalpy change (ΔH) is -14.0 kJ/mol.