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The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy 8, -210 kJ/mol. If the rate constant of this reaction is 1.2 x 10's 'at 101.0 °C, what will the rate constant be at 72.0°C? Round your answer to 2 significant digits. * -M'' х ?
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 82.0 °C 1.2 x 108 1.5 x 109 -1.0°C Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. Round your answer to 2 significant digits. kJ E. 0 D mol Х 5 ?
Some measurements of the initial rate of a certain reaction are given in the table below. [NL] [H] initial rate of reaction 2.14M 1.94M 70.0 Ms 0.827 M 1.94M 10.5 M/s 2.14M 0.604M 6.79 M/s Use this formation to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k0 D. Х 5 ?