Determining intial rates of reaction

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To determine the initial rate of the reaction between C2H5Br and OH-, the concentrations of both reactants are crucial, as they influence the rate according to the rate equation. The initial rate can be calculated using the formula rate = k[C2H5Br][OH], where k is the rate constant that varies with temperature. The provided concentrations of 0.16 M for C2H5Br and 0.26 M for OH- indicate that the reaction is not at equilibrium, as equilibrium would require equal concentrations. The activation energy and frequency factor may be relevant for calculating k at the specified temperature of 85 degrees. Understanding how to apply these concentrations in the rate equation is essential for accurately determining the initial reaction rate.
dnt
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problem states:

C2H5Br + OH- --> C2H5OH + Br-

if the reaction mixture is .16 M C2H5Br and .26 M OH-, then what is the intial rate of reaction at 85 degrees.

they also give a table of different temperatures and the associated k values at each. i also determined the activation energy and frequency factor for the reaction (if it matters at all for this question).

my main question is, is the fact that there are two different concentrations given make a difference in the answer? how do i use those numbers? shouldn't they be the same if the reaction is at equilibrium?
thanks
 
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What is rate equation?
 
i think i solved it:

rate = k[C2H5Br ][OH]

correct?
 

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