Rate law and reaction order | Kinetics | AP Chemistry | Khan Academy

A rate law shows how the rate of a chemical reaction depends on reactant concentration. For a reaction such as aA → products, the rate law generally has the form rate = k[A]ⁿ, where k is a proportionality constant called the rate constant and n is the order of the reaction with respect to A. The value of n is not related to the reaction stoichiometry and must be determined by experiment. View more lessons or practice this subject at www.khanacadem...
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I think it would be like if you multiplied [A] by 2 but the initial rate would remain the same.

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Why there is a difference in the order between different reactants?
Why there is a zero order or a first order .. etc

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[@garen5594]

Anyone know when to use this
average rate of reaction = (-1/a)(deltaA/deltat)
First order and second order
ln(k2/k1) = -Ea/R(1/t2-1/t1)

[@TMPChem]

Hi Garen. For a reactant "a" in a 1st order reaction, { -1/a d[A]/dt = k[A] }. This leads to the 1st order integrated rate law, { [A]_t = [A]_o exp( -a k t ) }. Your second equation comes from the Arrhenius equation { k = A exp( Ea / RT ) }, which describes the temperature dependence of the rate constant. If you plot the natural log of the rate constant versus the inverse of the temperature, you'll find a straight line whose slope is { -Ea / R }, the "activation energy" divided by the gas constant.

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At the end, shouldn't the units for k be mol/L*s ?

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Is rate always m/s or it can change?

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HELP! what if the one im trying to work out only has 1 table of initial rates? do i do what you did but compare A and B to that one table of initial rates?

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[@gersoncocjinjr.8566]

what if concentration [A] stays the same and the rate increased by 2 what would happen in that case

[@nightflares3572]

What u r talking about is impossible, bcz according to rate law, " (initial) rate of reaction " is dependent on "concentration of reactant", meaning that rate of reaction changes corresponding to change in concentration of reaction. There is no way that u keep the concentration of reactant same , but the rate of reaction changes. If it does, then rate of reaction is not in its initial stage ( meaning "t" will not be equal to 0), but some time will be passed after rate of reaction has started.

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