Reaction Rates and Temperature The rate constant of a chemical reaction increase

Question

Reaction Rates and Temperature The rate constant of a chemical reaction increased from 0.100 s temperature from 25.0 °C to 35.0 °C to 3.10 s upon raising the Learning Goal the Arrhenius equation to calculate the To use activation energy Part A As temperature rises, the average kinetic energy of molecules increases. In a chemical reaction, this means that a higher percentage of the molecules possess the required activation energy, and the reaction goes faster. This relationship is shown by the Arrhenius equation where Ti is the initial temperature and T2 is the final Calculate the value of temperature Express your answer numerically T2 T where k is the rate constant, A is the frequency factor, Ea is the activation energy, R 8.3145 J/ (K·mol) is the gas constant, and T is the Kelvin temperature. The following version of the equation is also 4 rearranged useful T2 Ti Submit Hints My Answers Give Up Review Part where ki is the rate constant at temperature T, and k2 is the rate constant at temperature T2 Incorrect Try Again; 2 attempts remaining

Explanation / Answer

ANSWER

(A) Convert the temperature to Kelvin scale

25oC = 298K

35oC = 308K

(1/T1 -1/T2) = (1/298K  -1/308K) = 0.0001

(C) The problem can be solved by Arrhenius equation

ln(K2/K1) = Ea/R (1/T1 -1/T2)

K2 = rate constant at temperature T2

K1 = rate constant at temperature T1

Ea = activation energy

R = Gas constant

ln(3.1/0.1) = Ea/R (1/T1 -1/T2)

3.45 = Ea/8.314 (1/298K -1/308K)

3.45 = (Ea/8.314) X0.0001

Ea = (3.45 X 8.314) / 0.0001 = 286,833J = 286.833KJ

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