Understanding Second-Order Reactions and the Rate Law Equation

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In summary, a "second-order reaction" typically refers to the overall order of the reaction being 2. This means that two reactants could each have an order of 1, or one reactant could have an order of 2 and the other have an order of 0. The rate equation for such a reaction would be r = k[x]^1[y]^1, which would result in a linear graph. However, in some cases, the term "second-order reaction" may be used to refer to the order of reaction relative to one of the reactants. It is important to clarify this distinction.
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iBill
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So say if someone is referring to a "second-order reaction", are they referring to the overall order of reaction being 2? So two reactants could have an order of 1, or one reactant could have an order of 2, and the other have an order of 0?

So say you have a rate equation that looks like this: r = k[x]^1[y]^1

Would this graph be a linear line? or would it be a curve?



So pretty much what I'm asking is if someone says "second order reaction" are they referring to the overall order of reaction, or the order of reaction relative to one of the reactants.

Thx in advance.
 
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Without further clarification it usually means overall. Sometimes you may hear it said like "first order in X", then it is not overall, but relative to reactant X. So for example "reaction is first order in X and first order in Y, second order overall".
 

What is a simple rate law?

A simple rate law is an equation that describes the relationship between the rate of a chemical reaction and the concentrations of the reactants. It is typically written in the form of Rate = k[A]^m[B]^n, where k is the rate constant and m and n are the reaction orders with respect to the reactants A and B, respectively.

How do you determine the rate constant in a simple rate law?

The rate constant (k) can be determined experimentally by conducting a series of experiments with varying initial concentrations of the reactants and measuring the corresponding reaction rates. By plotting the data and using the rate law equation, the value of k can be determined from the slope of the resulting graph.

What is the difference between the rate constant and the rate of a reaction?

The rate constant (k) is a constant value that is specific to a particular reaction. It represents the proportionality between the rate of the reaction and the concentrations of the reactants. The rate of a reaction, on the other hand, is the change in concentration of a reactant or product over time. It is dependent on the rate constant as well as the initial concentrations of the reactants.

What is the reaction order in a simple rate law?

The reaction order refers to the exponent (m or n) in the rate law equation. It represents the effect of the concentration of a particular reactant on the rate of the reaction. A reaction order of 1 means that the rate is directly proportional to the concentration of that reactant, while a reaction order of 0 means that the concentration has no effect on the rate.

Can the rate law change during a reaction?

No, the rate law remains constant throughout a reaction. However, the rate itself may change as the concentrations of the reactants and products change. This can be observed by measuring the rate at different time intervals during the reaction.

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