Rate of Reaction: 3A + 5B --> 4C + 2D

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In the reaction 3A + 5B → 4C + 2D, the rate of reaction is expressed as r = k[A]^3[B]^5, indicating it is an elementary process. The confusion arises regarding the rate of production of A, which is stated to be three times the rate of reaction. This is because the stoichiometry of the reaction indicates that for every mole of reaction, three moles of A are consumed, affecting the rate of production. Thus, the rate of production of A is indeed three times the rate of reaction, as it reflects the consumption of three moles per reaction event. Understanding this relationship clarifies the dynamics of reaction rates in chemical processes.
quietrain
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3A + 5B ----> 4C + 2D

if this is an elementary process

the rate of reaction is given as

r = k [A]3 [ B ]5 , where k is rate constant, [x] are concentrations

so my question is , why is the rate of production of A = 3 times the rate of reaction?

since the rate of reaction has already taken into account the 3 moles of A, shouldn't the rate of production of A = rate of reaction ?

thanks!
 
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