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An irreversible reaction A + B  products is studied under conditions where the initial concentrations...

An irreversible reaction A + B  products is studied under conditions where the initial concentrations of A and B are equal. Under these circumstances, a graph of ln([A]) as a function of time is linear. What is the order in A?

(A) Zeroth order

B) First order

(C) Second order

(D) The order in A cannot be determined based on the information given.

Doesn't the first order reaction kinetics say that the graph of ln[A] vs t gives a straight line if the reaction is in first order? The form of the equation in ln[A] = -kt + ln[A0]. This tells us that the reaction is in first order with k as the rate constant. So why can't the order be determined based on the given information? Please explain how this question defies first order reaction kinetics. Another response that I got was that the graph could have a positive slope, but that wouldn't be possible as the concentration of the reactent must decrease! Please help. Thanks

Note: The correct answer is D not B. I am confused as to why the answer is D and not B. Can someone please explain? The answer is not B. It is D.

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