The following reaction is studied in the laboratory: 3X4 → 12Y8 + 4Z It is determined that at 111 °C, the rate constant of the reaction is 0.000812 L-mol-1-s-1. The activation energy is equal to 83300 J/mol. What will be the rate constant of the reaction at 36°C? Note: T(K) = T(°C) + 273 Give an answer with 4 significant figures.

Ethyl iodide decomposes to give ethylene and hydrogen iodide in thefirst order gas-phase reaction C2H5I → C2H4 + HI At 600 K, the value of k is determined to be 1.6 x 10-6 s^-1When the temperature is raised to 700 K, the value of k increases to 6.36x10-3 s^-1What is the activation energy of the reaction?

The reaction C,H3 (g) → 2C,H,(g) 4. has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 × 10-8 s-'. What is the value of the rate constant at 830.0 K? k = * TOOLS x10

For a certain reaction, the activation energy is found to be (1.77x10^1) kJ/mol. If the rate constant is (3.6x10^-5) at (3.78x10^2) K, what is the rate constant at (6.290x10^2) K?   R = 8.314 J/Kmol;     T(K) = T(°C) + 273 Report your answer in the same units as k1, with 2 sig figs.

Calculate the rate constant at 168 °C for a reaction that has an activation energy, EA = 21.1 kJ/mol and a rate constant, k = 0.0518 s1 at 28.8 °C. R = 8.314472 J• mor1. K-1. Report your answer to THREE significant figures.

The reaction C 4 H 8 (g) longrightarrow2C 2 H 4 (g) has an activation energy of 262kJ / m * o * l . At 600.0 K, the rate constant, k, is 6.1 * 10 ^ - 8 * s ^ - 1 What is the value of the rate constant at 800.0 K? k=

The rate equation for the hydrolysis of sucrose to fructose and glucose C₁2H₂O(aq) + H₂O()→ CsH₁2Os(aq) + CH₂Os (aq) is-A[sucrose]/At=k[C₁₂H₂O₂). After 28 minutes at 27 °C, the sucrose concentration decreased from 0.0112 M to 0.0090 M. Find the rate constant k. k= min-1 Submit Answer Try Another Version 4 item attempts remaining

For the reaction A + B ---> C, the rate constant at 215°C is 5.0x10-3 M-1s-1and 1.2x10-1  M-1s-1at 452 °C. What is the activation energy for the reaction? [R=8.314 x 10-3kJ/mol.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.

For the interconversion between A and B as shown below, which of the following describes how the equilibrium constant (K) is related to the rate constants k1 and k -1 and to the amounts of A and B present at equilibrium? k1 A В k.1 OK = kj[A] and K = kj[B] k[B] K = kj[A] [B] K and K || [A] k1 [B] [A] K and K %3D k-1 k[A] K = kj[B]