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Kinetics动力学
Thermodynamics determines whether and in which direction a reaction will happen, and what the concentrations of constituents are involved in the reaction
热力学决定了反应是否发生、反应的方向以及参与到反应之中的物质浓度问题。
Kinetics say how fast a reaction happens, sequence of steps in the reaction, and some of the factors that control the rates of reactions
动力学则说明反应发生的速率有多快、反应步骤的顺序以及控制反应速率的一些因素
Further Reading (Chapter 3 in Hobbs)
Rate of reaction is typically measured as the
change in concentration (moles/L) with time
反应速率通常通过浓度(mol/L)随时间的变化来测量
This change may be a decrease or an increase
改变可能是增加的也可能是减小的
Likewise the concentration change may be of
reactants or products
同样,改变浓度的物质可能是反应物也可能是生成物
反应速率=△浓度/△时间
Rate has units of moles per liter per unit time
- M s-1, M h-1
速率的单位是摩尔每升每单位时间,如M s-1、M h-1
Consider the hypothetical reaction
对于这个假设的反应
aA + bB cC + dD
We can write
Note the use of the negative sign
注意负号的使用
- rate is defined as a positive quantity
反应速率被定义为正量
- rate of disappearance of a reactant is
negative
那么,反应物的消耗速率就是负的
2N2O5(g) 4NO2(g) + O2(g)
Rate may be expressed in three main ways:
反应速率主要有以下三个表达方式:
Average reaction rate: a measure of the
change in concentration with time
1、平均反应速率:浓度随时间变化的度量
2. Instantaneous rate: rate of change of
concentration at any particular instant during the
Reaction
2、瞬时速率:反应过程中某一特定瞬间的浓度变化速率
3. Initial rate: instantaneous rate at t = 0
- that is, when the reactants are first
mixed
3、初始速率:t=0时即反应物最初混合时的瞬时速率,
Rate Laws 速率定律
Rate law = a mathematical function describing the turnover rate of the compound of interest as a function of the concentrations of the various species participating in the reaction
速率定律:用来描述相关的化合物的转化速率的数学函数,即各种参与反应的物质的浓度的函数
May or may NOT have a theoretical basis可能有或没有理论基础
“Many reactions occur at a decreasing rate with increasing time because the reaction rate diminishes as the concentrations of the reactants diminish”
“很多反应随着时间的增加反应速率逐渐减小?,因为反应物浓度减小会降低反应速率”
Hobbs (2000)
Rate Laws
“m” indicates
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