The rate constant k for a certain reaction is measured at two different temperatures: temperature k 7 286.0 °C 6.5 × 10' 169.0 °C 4.2 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 mol

Some measurements of the initial rate of a certain reaction are given in the table below. H2 2 initial rate of reaction 1.10M| 2.49M 9.00 x 10°M/s 3.05M 2.49М 2.50 x 10*M/s 1.10M 6.51M 2.35 x 10*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 = ?

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 381.0 °C 5.1 x 10⁹ 321.0 °C 2.6 × 10⁹ 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 U E = a mol Ś ? 0 x10 X

Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 215.0 °C 3.7 x 107 134.0 °C 1.4 x 106 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 = 0 mol ? 0 x10 X

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 59.0 °C 6.5 x 101 14 163.0 °C |4.2 × 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 x10 mol

A certain catalyzed reaction is Known to have an activation energy Ea=29.0 kJ/mol. Furthermore, the rate of this reaction is measured at 331 K and found to be 2.7× 10* M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is raised by 10% from 331 K to 364 K. How will the rate or the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed which has the eftect of raising the activation energy by 10%, from 29.0 kJ/mol to 31.9 kJ mol How will the rate or the reaction change?

Consider this reaction.    2A             B     It obeys the rate law:    rate =   k [A] 2   and  k = 0.188 M -1 s -1 If the initial concentration of A is 0.600 M, at what time will the concentration be 50.0% of that value? Consider this reaction.    2A             B     It obeys the rate law:    rate =   k [A] 2   and  k = 0.188 M -1s -1 If the initial concentration of A is 0.600 M, at what time will the concentration be 50.0% of that value? 793 s 8.87 s 182  s 9.48 x 103 s 79.1 s 3.07 x 10-3 s 1.50 x 109 s 5.22  x 10-2 s

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 278.0 °C 207.0 °C Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. Ea 2.1×10⁹ 4.5×108 kJ mol x10 X

The rate constant for the formation of hydrogen iodide from the elements H₂(g) + 1₂(g) → 2Hİ(g) is 2.7 x 10-4 L/(mol-s) at 600 K and 3.5 x 10-3 L/(mol·s) at 650 K. a. Find the activation energy Ea. J/mol b. Then calculate the rate constant at 719 K. L/(mol.s)