Determining intial rates of reaction

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SUMMARY

The discussion focuses on calculating the initial rate of the reaction between C2H5Br and OH- at a concentration of 0.16 M C2H5Br and 0.26 M OH- at 85 degrees Celsius. The user correctly identifies the rate equation as rate = k[C2H5Br][OH], where k is the rate constant. The presence of different concentrations does affect the initial rate calculation, as the rate depends on the concentrations of both reactants. The activation energy and frequency factor, while relevant for understanding the reaction kinetics, are not necessary for determining the initial rate in this context.

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  • Understanding of chemical kinetics and rate laws
  • Familiarity with the Arrhenius equation for activation energy
  • Knowledge of concentration units in molarity (M)
  • Basic principles of equilibrium in chemical reactions
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Chemistry students, researchers in chemical kinetics, and anyone interested in understanding reaction rates and their dependence on concentration and temperature.

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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