对比氧化潜在演变和上限管理技术对红葡萄酒化学成分的影响
Dallas J Parnigoni1, Sean T Kuster1, Jesus Villalobos1
1Wine and Viticulture Department, California Polytechnic State University San Luis Obispo (Cal Poly), San Luis Obispo, CA 93407, USA.
Molecules (Basel, Switzerland)
|August 14, 2025
概括
管理葡萄酒盖的氧化还原潜力会影响葡萄酒的成分. 惰性气体改善了化合物,而空气可能会减轻凝聚力,而谷氨酸比率表明了氧化还原史.
科学领域:
- 葡萄酒学 葡萄酒学 葡萄酒学
- 葡萄酒化学 葡萄酒化学
- 发酵科学 发酵科学
背景情况:
- 氧化降低潜力 (ORP) 在发酵过程中影响葡萄酒的质量.
- 酒顶管理技术会影响葡萄酒的化学和感觉特征.
研究的目的:
- 调查六个帽子管理协议对Pinot noir葡萄酒发酵的影响.
- 分析不同氧化降低潜力 (ORP) 演变如何影响葡萄酒的组成和质量.
主要方法:
- 测试了六种帽子管理协议:打孔下降 (PD),转 (PO),空气/N2注射 (AirMix,N2Mix) 和ORP触发的空气/N2注射 (RedoxConAir,RedoxConN2).
- 测量包括ORP,谷氨氧化还原状态 (GSH:GSSG比率),总基,素,-3-ols和挥发性成分.
主要成果:
- 艾米克斯葡萄酒 (ORP>0mV) 具有较低的和氨酸,但具有氧化有利的GSH:GSSG比率 (0.3:1).
- N2Mix葡萄酒 (ORP ≈ -100 mV) 显示了减少偏好的GSH:GSSG比率 (7:1).
- PD葡萄酒的产量比PO葡萄酒高出48%的flavan-3-ols;在不同处理方法中,乙烯-n-octanoate的产量有显著差异.
结论:
- GSH:GSSG比率可以表明葡萄酒在发酵过程中的氧化还原史.
- 帽子管理策略显著影响葡萄酒的含量,颜色和挥发性香味特征.
- 惰性气体注射维持或增加了含量,而空气注射可能会减少性.
相关概念视频
Ladder Diagrams: Redox Equilibria
529
Ladder diagrams are useful tools for understanding redox equilibrium reactions, especially the effects of concentration changes on the electrochemical potential of the reaction. The vertical axis in the redox ladder diagrams represents the electrochemical potential, E. The area of predominance is demarcated using the Nernst equation.
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...
529
Redox Titration: Overview
3.4K
Redox titration is a chemical analysis technique used to determine the concentration of an unknown substance by measuring the electron transfer in a redox (reduction-oxidation) reaction. The process involves gradually adding a titrant with a known concentration of an oxidizing or reducing agent, to the analyte, the solution with an unknown concentration, until reaching the endpoint, which indicates the completion of the reaction between the two substances. Ensuring the analyte is in a single...
3.4K
Redox Equilibria: Overview
993
A reduction-oxidation reaction is commonly called a redox reaction. In a redox reaction, electrons are transferred from one species to another rather than being shared between or among atoms. The reducing agent or reductant is the species that loses electrons and gets oxidized in the process. The species that gains electrons and gets reduced in the process is the oxidizing agent or oxidant. Redox reactions are represented as two separate equations called half-reactions, where one equation...
993
Redox Titration: Other Oxidizing and Reducing Agents
393
Besides iodine, other oxidizing or reducing agents can serve as titrants in redox titrations. Common oxidizing titrants include KMnO4, cerium(IV), and K2Cr2O7. The choice of oxidizing titrants depends on factors like stability, cost, analyte strength, and reaction rate between the analyte and titrant. KMnO4 is a strong oxidizing titrant that reduces from Mn(VII) to Mn(II) in a highly acidic solution, simultaneously oxidizing the analyte to a higher oxidation state. In this case, KMnO4 acts as a...
393
Voltammetry: Factors Affecting Measurements
207
A current produced due to the redox reactions of the analyte at the working and auxiliary electrodes is called a faradaic current. The reaction can be divided into two types. The current generated due to the reduction of the analyte is called cathodic current, and it carries a positive charge. In contrast, the current produced by analyte oxidation is known as an anodic current, and it has a negative charge. The applied potential at the working electrode determines the faradaic current flow, and...
207
The Nernst Equation
42.2K
Nonstandard Reaction Conditions
The interconnection between standard cell potentials and various thermodynamic parameters such as the standard free energy change ΔG° and equilibrium constant K has been previously explored. For example, a redox reaction involving zinc(II) and tin(II) ions at 1 M concentration with Eºcell = +0.291 V and ΔG° = −56.2 kJ is spontaneous.
The interconnection between standard cell potentials and various thermodynamic parameters such as the standard free energy change ΔG° and equilibrium constant K has been previously explored. For example, a redox reaction involving zinc(II) and tin(II) ions at 1 M concentration with Eºcell = +0.291 V and ΔG° = −56.2 kJ is spontaneous.
42.2K


