The rate constant k for a certain reaction is measured at two different temperatures: temperature k 5.9 x 107 |3.5 × 106| Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. 73.0 °C - 12.0 °C

59.  The rate constant for the decomposition of acetaldehyde, CH3CHO, to methane, CH4, and carbon monoxide, CO, in the gas phase is 1.1 × 10−2 L mol−1 s−1 at 703 K and 4.95 L mol−1 s−1 at 865 K. Determine the activation energy for this decomposition.

An energy diagram showing two peaks suggests that there are two steps and three transition states in the reaction mechanism. Select one: O True O False Given a reaction with an activation energy of 2.3 x 104 J/mol. The rate constant will increase by a factor of when the reaction temperature is increased from 200 °C to 250 °C. O 2.42 O 2.81 O 1.58 O 1.75 For the complete neutralization reaction between a 1 M strong acid and a 1 M strong base of equal initial volumes that is marked by a temperature rise, the entropy of neutralization is positive (ASn > 0) whereas the Gibbs free energy is negative (AGxn < 0). Select one: O True O False

16.  The decomposition of hydrogen bromide is 2 HBr(g)    →    H2(g)  +  Br2(g) The reaction has rate constants of 7.23 x 10-8 M-1 s-1 at 5.00 x 102 K and 9.14 x 10-6 M-1 s-1 at 6.00 x 102 K. What  is the activation energy in kJ/mol? Group of answer choices 136 kJ/mol none of the answers are correct 145 kJ/mol 107 kJ/mol 121 kJ/mol

A certain catalyzed reaction is known to have an activation energy E= 11.0 kJ/mol. Furthermore, the rate of this reaction is measured at 296. K and found to be 1.1 × 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 296. K to 326. K. How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed, which has the effect of raising the activation energy by 5%, from 11.0 kJ/mol to 11.6 kJ/mol. How will the rate of the reaction change? The rate will The rate will choose one choose one choose one stay the same rise about 5% rise more than 5% rise less than 5% fall about 5% fall more than 5% fall less than 5% V

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

The activation energy for the following reaction is 125 kJ/mol, and AE for the reaction is -216 kJ/mol. NO₂(g) + CO(g) → NO(g) + CO₂(g) What is the activation energy for the reverse reaction NO(g) + CO₂(g) → NO₂(g) + CO(g) Please enter your answer as a real number only. (The units should be kJ/mol, but leave that off. Just enter a number like 420.3. But don't enter 420.3. Enter the correct answer.)

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?

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 132.0 °C E Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. a Round your answer to 2 significant digits. a 242.0 °C = 6.2 × 10¹1 3.8 × 10¹3 kJ mol x10

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