The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 48.0 kJ/mol. If the rate constant of this reaction is 7.9 x 10³ M -1 at 218.0 °C, what will the rate constant be at 186.0 °C? Round your answer to 2 significant digits. -1 -1 k= = :5 X Ś 4

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 248.0 °C 9.9 x 108 169.0 °C 9.8 x 107 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 X S ?

When a reaction is performed at a temperature of 314. K, the rate constant is 1.9 x 10-6 s-1. When performed at 457. K, the rate constant is 8.5 x 104s-1. Calculate the activation energy_(Ea) of this reaction, in units of kJ/mol.

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.

Sketch a potential energy diagram for the decomposition of nitrous oxide. N2O(g) →→ N2(g) + O(g) The activation energy for the forward reaction is 171  kJ;  If the activation energy for the reverse reaction is 99 kJ, calculate the standard enthalpy change for this reaction.  Transfer all the information into an energy diagram.   label appropriately

What is the activation energy of a reaction if it has the following rate constants?

When heated, cyclopropane is converted to propene. Rate constants for this reaction at 470. °C and 510. °C are k1 = 1.10 × 10-4 s-1 and k2 = 1.02 × 10-3 s-1, respectively. Determine the activation energy, Ea, from these data. Ea =  kJ/mol

The rate constant k for a certain reaction is measured at two different temperatures: temperature 311.0 °C E = a 246.0 °C Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. a Round your answer to 2 significant digits. 0 kJ k 1.4 × 10¹⁰ 2.0 × 10⁹ mol x10 × S

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 407.0 °C 4.8 x 10¹0 268.0 °C 2.3 × 10 ¹0 a 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 X 3 ?