Orders
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Re: Orders
the total order of the reaction is the sum of the exponential coefficients. This can be determined based on graphs, a given rate law, or an integrated rate law.
Re: Orders
the order can also be determined by the given rate constant and the units or from a table with given concentrations and rates
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Re: Orders
A first-order reaction means that there is one reactant or molecule present in the rate law. A second-order rate law either has two of the same reactant (rate law would be squared) or two different ones (they would be multiplied by each other). Two examples of second-order reactions are rate=k[CO2]^2 or rate=k[CO2][H2O].
Re: Orders
asannajust_1J wrote:the total order of the reaction is the sum of the exponential coefficients. This can be determined based on graphs, a given rate law, or an integrated rate law.
Would the graphs be given to us?
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Re: Orders
I believe that if we need to determine the order of a reaction based on graphs, then they will most likely provided the graphs that we need.
Re: Orders
How would we know the order of the reaction if we are given an integrated rate law?
asannajust_1J wrote:the total order of the reaction is the sum of the exponential coefficients. This can be determined based on graphs, a given rate law, or an integrated rate law.
Re: Orders
As far as I know, we never include products in the rate law, correct?
Brianna Becerra 1B wrote:A first-order reaction means that there is one reactant or molecule present in the rate law. A second-order rate law either has two of the same reactant (rate law would be squared) or two different ones (they would be multiplied by each other). Two examples of second-order reactions are rate=k[CO2]^2 or rate=k[CO2][H2O].
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Re: Orders
Timmy Nguyen Dis 1I wrote:How do we know which order the reaction is?
You can use the given rate constant and the units or from a table with given concentrations and rates.
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