How to Differentiate Between First Order and Second Order Processes?

Thread starter Emy.Hady
Start date Dec 17, 2011
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First order

In summary, first order reactions have a rate directly proportional to the concentration of one reactant, while second order reactions have a rate directly proportional to the concentration of two reactants. Examples of first order reactions include radioactive decay, hydrolysis of esters, and decomposition of hydrogen peroxide. The rate law for a first order reaction can be determined by plotting the natural logarithm of the concentration of the reactant against time and finding the slope, which is equal to the rate constant. The half-life of a first order reaction is constant and can be calculated using the equation t1/2 = 0.693/k where t1/2 is the half-life and k is the rate constant. A second order reaction cannot have a rate

Dec 17, 2011

Emy.Hady

How can i differentiate between first order & second order ??!

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Dec 17, 2011

Borek

Mentor

http://en.wikipedia.org/wiki/First_order

http://en.wikipedia.org/wiki/Second_Order

And you expect us to know what you are asking about? Sorry, we are not mind readers.

FAQ: How to Differentiate Between First Order and Second Order Processes?

What is the difference between first order and second order?

First order refers to the rate of a chemical reaction being directly proportional to the concentration of one reactant. Second order refers to the rate of a chemical reaction being directly proportional to the concentration of two reactants.

What are some examples of first order reactions?

Some examples of first order reactions include radioactive decay, hydrolysis of esters, and the decomposition of hydrogen peroxide.

How do you determine the rate law for a first order reaction?

The rate law for a first order reaction can be determined by plotting the natural logarithm of the concentration of the reactant against time and finding the slope of the resulting line. The slope will be equal to the rate constant for the reaction.

What is the half-life of a first order reaction?

The half-life of a first order reaction is constant and can be calculated using the equation t1/2 = 0.693/k, where t1/2 is the half-life and k is the rate constant.

Can a second order reaction have a rate constant with units of M/s?

No, the rate constant for a second order reaction will have units of 1/(M*s) or M^-1*s^-1. This is because the rate of a second order reaction is dependent on two reactants, so the units will reflect this dependency.