Which of the following is the correct rate expression for the forward reaction aA + bB <----> cC +dD ?
A. Q = [A]a x [B]b
B. Q = [A] x [B]
C. Q = k1 x [A]a x [B]b
D. Q = r1 x [A]a x [B]b
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@Aqhex = [A] x [B]
don't you need the number of moles as powers?
i have no clue i just gather answer and info
you can't deduce the rate law expression from the balanced reaction alone, you need experimental data.
@aaronq That may be true, but yet the student was asked to find the correct rate expression. Perhaps part of the problem is missing, such as the order of the reaction with respect to the products. Is it not the case that if we knew the order of the reaction we would be able to determine the correct form?
It's possible to determine the right rate law if given a limited number of options, because if the question indicated a second order then we could have both reactants in the first order (each) or only one of the reactants in the second order.
\(rate=k[A][B]\) or \(rate=k[A]^2\) or \(rate=[B]^2\)
frig, i missed the rate constant in the last one.
The rate law is experimentally determined
You must have a rate constant too in the rate law in the form k1[A][B] = r