The rate constant & for a certain reaction is measured at two different temperatures: temperature k 81.0 °C 4.0×10¹¹ 137.0 °C 1.6×10¹2 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reactio Round your answer to 2 significant digits. mol x10 X

Some measurements of the initial rate of a certain reaction are given in the table below. [H,] 2 initial rate of reaction 1.50M 0.382М 20.0M/s 3.30M 0.382м 44.0M/s 1.50M| 0.647M 33.9 M/s Use this information 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 = k || x10 k =

A student collected conducted 6 kinetics experiments for one reaction by holding the concentrations of ALL the reactants and catalyst constant and varying the temperature. After determining the rate constant for this reaction at the 6 different temperatures, an Arrhenius Plot was made. The graph resulted in a straight line. The equation for the straight line was: y= -4,257.15 x + 14.326 What is the Activation Energy (in Joules/mol) for this reaction at 30 oC? Do not include the units in your answer.

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 401.0 °C 5.2 x 10° 270.0 °C |2.7 × 10° Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. Round your answer to 2 significant digits. E Ox10 %3D mol

Q1. Which of the following reactions will be the fastest to be complete? Q2. Discuss each factors that will affect the rate of reaction to receive full points. Factors Reaction #1 Reaction #2 Reaction #3 Reactant 5 M 5 M 5 M Concentration Surface Area Small Large Large Temperature 25 °C 35 °C 20 °C Catalysts Yes Yes No

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 330.0 °C 3.6 × 10 264.0 °C 1.3 × 10* Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. a Round your answer to 2 significant digits. kJ E a mol

A certain reaction has an activation energy of 43.99 kJ/mol. At what Kelvin temperature will the reaction proceed 4.00 times faster than it did at 353 K?

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 204.0 °C 1.1 × 107 103.0 °C 1.3 × 10° Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. а Round your answer to 2 significant digits. kJ E %D a mol

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 61.0 °C 6.7 x 10° -76.0 °C 4.5 x 10* 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 x10 a mol II

Some measurements of the initial rate of a certain reaction are given in the table below. |H2|| ||2| | initial rate of reaction 1.50M| 2.25М 0.540 M/s 1.50M 6.45 М 1.55 M/s 5.57 М 2.25М 2.01 M/s Use this information 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 = k x10 k =