Areaction is followed and found to have a rate constant of 3.36 × 104 m-1s-1 at 344 k and a rate constant of 7.69 m-1s-1 at 219 k. determine the activation energy for this reaction. a reaction is followed and found to have a rate constant of 3.36 × 104 m-1s-1 at 344 k and a rate constant of 7.69 m-1s-1 at 219 k. determine the activation energy for this reaction. 12.5 kj/mol 11.5 kj/mol 23.8 kj/mol 58.2 kj/mol 42.0 kj/mol

The relation between rate constants at different temperatures, temperature and activation energy is known as Arrhenius equation

Arrhenius equation

For two temperatures

Where

Ea = ? = activation energy

k1 = 3.36 × 10⁴

T1=344 k

k2=7.69

T2=219K

R= gas constant = 8.314 J /molK

Putting values

Ea = (-69.69)/(-0.00166) = 41981.93 J/mol

Or

Activation energy is 42.0 kJ /mol

the answer is a and have a great day

here is table 2-2:

country

percent of eligible voters that voted

rank

united states

44.9%

138

canada

60.1%

107

costa rica

84.6%

14

hungary

66.9%

82

japan

57.0%

118

egypt

27.7%

159

south africa

85.5%

10

ans is no, the data set cannot be plotted as a single circle graph