Second Order Reactions
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Second Order Reactions
What determines a reaction as a second order reaction and not as a first order reaction?
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Re: Second Order Reactions
In a first order reaction, there will be one reactant present in the rate law. For a second order reaction, you can either have a rate law with one reactant to the second order, or with two reactants both to the first order.
Found this answer (and others) here: https://lavelle.chem.ucla.edu/forum/viewtopic.php?t=28639
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- Posts: 101
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- Posts: 100
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Re: Second Order Reactions
One way is to graph the reaction and see which equation results in a linear graph. A linear graph that plots [R] to time is zero order, ln[R] to time is first order, and 1/[R] to time is second order.
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Re: Second Order Reactions
A second-order reaction (where order = 2) has a rate proportional to the concentration of the square of a single reactant or the product of the concentration of two reactants. The formula is:
rate = k[A]2 (or substitute B for A or k multiplied by the concentration of A times the concentration of B), with the units of the rate constant M-1sec-1
For a first order reaction, the rate law would be = k[A] (or B instead of A), with k having the units of sec-1
rate = k[A]2 (or substitute B for A or k multiplied by the concentration of A times the concentration of B), with the units of the rate constant M-1sec-1
For a first order reaction, the rate law would be = k[A] (or B instead of A), with k having the units of sec-1
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Re: Second Order Reactions
Where in the book can we find examples of first and second order reactions?
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