The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=51.0 kJ/mol. If the rate constant of this a 1 -1 reaction is 6.2 × 10° M 'S at 156.0 °C, what will the rate constant be at 202.0 °C? Round your answer to 2 significant digits.

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 54.0 kJ/mol. If the rate constant of this reaction is 2.0 × 10³ M¹s -1.-1 at 222.0 °C, what will the rate constant be at 272.0 °C? Round your answer to 2 significant digits. k = M .S Ś 囧

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E, = 8.0 kJ/mol. If the rate constant of this reaction is 1.1 x 10° M -1 -1 'S at 160.0 °C, what will the rate constant be at 108.0 °C? Round your answer to 2 significant digits.

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=11.0 kJ/mol. If the rate constant of this a 1 - 1 reaction is 3.2 × 10° M S. at 112.0 °C, what will the rate constant be at 149.0 °C? Round your answer to 2 significant digits. 1 - 1 k = ] M x10 •S ?

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 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.)

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=69.0 kJ/mol. If the а - 1 rate constant of this reaction is 5.7 × 10² M - 1 S. at 304.0 °C, what will the rate constant be at 256.0 °C? Round your answer to 2 significant digits. - 1 - 1 k = || M •S x10 ?

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E, = 9.0 kJ/mol. If the rate constant of this reaction is 1.1 x 10 M 's -1 at 226.0 °C, what will the rate constant be at 146.0 °C? 10° Round your answer to 2 significant digits.

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 258.0 °C 3.9 x 1010 153.0 °C 1.5 × 1010 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 х10 a mol

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=77.0 kJ/mol. If the rate constant of this reaction is 5.5 × 10 4 1 M S. at 55.0 °C, what will the rate constant be at 16.0 °C? -1 Round your answer to 2 significant digits. 1 1 k = ]Ms •S