酵素の計算による熱安定化.
Aaron Korkegian1, Margaret E Black, David Baker
1Division of Basic Sciences, Fred Hutchinson Cancer Research Center (FHCRC), 1100 Fairview Avenue North, Seattle, WA 98109, USA.
まとめ
コンピューティング・メソッドは,3つの酵素変異を迅速に特定しました. これらの変異は,触媒効率を損なうことなく,熱安定性と半減期を大幅に増加させ,細菌の増殖を可能にしました.
科学分野:
- 酵素工学とは,酵素工学である.
- 計算生物学とは,計算生物学である.
- メタボリックエンジニアリング
背景:
- 工業用途の酵素の熱安定化は,従来の方法では困難です.
- 高温で酵素の活性を維持することは,多くのバイオテクノロジーのプロセスにとって極めて重要です.
研究 の 目的:
- 酵素の熱安定化のための急速な計算アプローチを開発する.
- 酵素の安定性と活性性を高める特定の突然変異を特定する.
- 分子工学と代謝工学の結合効果を実証するために.
主な方法:
- モデル酵素の変異を特定するために,急速な計算戦略を利用した.
- 酵素に3つの特定の変異を導入した.
- 50°Cでの表面溶解温度 (Tm) と半減期の変化を評価した.
- 酵素の触媒効率を評価した.
- 温度に依存する条件下で測定された細菌の成長率.
主要な成果:
- Tmを10°C増加させる3つのシナージスティック変異を特定した.
- 50°Cで酵素半減期を30倍に増加させました.
- 酵素の触媒効率の低下は観察されなかった.
- 温度に依存するバクテリアの成長率の増加を示した.
結論:
- 急速なコンピューティングアプローチにより,熱安定酵素を効果的に設計することができます.
- 合成変異は酵素の安定性と機能を高めます.
- エンジニアリングされた酵素は,温度に依存した方法で代謝パフォーマンスを改善することができます.
関連する概念動画
Calculating the Equilibrium Constant
The equilibrium constant for a reaction is calculated from the equilibrium concentrations (or pressures) of its reactants and products. If these concentrations are known, the calculation simply involves their substitution into the Kc expression.
For example, gaseous nitrogen dioxide forms dinitrogen tetroxide according to this equation:
For example, gaseous nitrogen dioxide forms dinitrogen tetroxide according to this equation:
Calculating Equilibrium Concentrations
Being able to calculate equilibrium concentrations is essential to many areas of science and technology—for example, in the formulation and dosing of pharmaceutical products. After a drug is ingested or injected, it is typically involved in several chemical equilibria that affect its ultimate concentration in the body system of interest. Knowledge of the quantitative aspects of these equilibria is required to compute a dosage amount that will solicit the desired therapeutic effect.
A more...
A more...
Calculating Standard Free Energy Changes
The free energy change for a reaction that occurs under the standard conditions of 1 bar pressure and at 298 K is called the standard free energy change. Since free energy is a state function, its value depends only on the conditions of the initial and final states of the system. A convenient and common approach to the calculation of free energy changes for physical and chemical reactions is by use of widely available compilations of standard state thermodynamic data. One method involves the...
The Nernst Equation
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.
Non-equilibrium in the Cell
An important concept in studying metabolism and energy is that of chemical equilibrium. Most chemical reactions are reversible. They can proceed in both directions, releasing energy into their environment in one direction, and absorbing it from the environment in the other direction. The same is true for the chemical reactions involved in cell metabolism, such as the breaking down and building up of proteins into and from individual amino acids, respectively. Reactants within a closed system...
Thermodynamics: Activity Coefficient
Activity is the measure of the effective concentration of the species in solution. It can be expressed as the product of the molar concentration of the species and its activity coefficient. The activity coefficient is a dimensionless quantity and depends on the total ionic strength of the solution.
The activity coefficient is a measure of the deviation from ideal behavior. When the ionic strength of the solution is minimal, the activity coefficient of an ionic species is close to unity, making...
The activity coefficient is a measure of the deviation from ideal behavior. When the ionic strength of the solution is minimal, the activity coefficient of an ionic species is close to unity, making...


