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The kinetics of the following second-order reaction were studied asa function of temperature:

C2H5Br (aq) + OH- (aq) -----> C2H5OH (l) + Br- (aq)

Temperature (C) k (L/mol*s)
25 8.81*10^- 5
35 0.000285
45 0.000854
55 0.00239
65 0.00633


If a reaction mixture is 0.155 M in C2H5Br, and 0.240 M in OH^ -,what is the initial rate of the reaction at 85 degrees C?

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Nestor Rutherford
Nestor RutherfordLv2
18 Apr 2019

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Related questions

99. The kinetics of this reaction were studied as a function of tem- perature. (The reaction is first order in each reactant and second order overall.) CH,Br(aq) + OH-(aq) = C,H,OH(I) + Br-(aq) & Temperature (°C) k (L/mol-) 8.81 x 10-5 35 0.000285 45 0.000854 0.00239 0.00633 a. Determine the activation energy and frequency factor for the reaction. b. Determine the rate constant at 15 °C. c. If a reaction mixture is 0.155 M in C2H5Br and 0.250 Min OH, what is the initial rate of the reaction at 75 °CCLIVA Go to se &

The kinetics of the following second-order reaction were studied as a function of temperature:
C2H5Br(aq)+OH−(aq)→C2H5OH(l)+Br−(aq)

Temperature (∘C) k (L/mol⋠s)
25 8.81×10−5
35 0.000285
45 0.000854
55 0.00239
65 0.00633

Part A: Determine the activation energy for the reaction.

Part B: Determine the frequency factor for the reaction.

Part C: Determine the rate constant at 10 ∘C.

Express your answer using two significant figures.

Part D: If a reaction mixture is 0.145 M in C2H5Br, and 0.250 M in OH−, what is the initial rate of the reaction at 90 ∘C?

Express your answer using two significant figures.

The reaction between ethyl bromide (C2H5Br) and hydroxide ion in ethyl alcohol at 330 K, C2H5Br(alc)+OH?(alc)?C2H5OH(l)+Br?(alc), is first order each in ethyl bromide and hydroxide ion. When [C2H5Br] is 0.0477 M and [OH?] is 0.100 M, the rate of disappearance of ethyl bromide is 1.7

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