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Arrhenius Equation

Q. What is the activation energy for a reaction if k = 1.89 x 10^-8 s^-1 at 540 K and k = 2.45 x 10^-7 s^-1 at 601 K? a. 113 kJ/mol b. 83 kJ/mol c. 410 kJ/mol d. 280 kJ/mol e. 580 kJ/mol

Solved • Jul 1, 2019

Arrhenius Equation

Q. What is defined as the minimum amount of energy required to initiate a chemical reaction? a. collision energy b, effective collision energy c. reaction energy d. activation energy e. rate energy

Solved • Jul 1, 2019

Arrhenius Equation

Q. The rate constant of a particular first order reaction is 5.45 x 10^-2 secA-1 at 40.0 oC. What is the rate constant of this reaction at 65.0 oC if the energy of activation, Ea for this reaction is 65.5 kJ/mol? 3.96 1.18 x 10^2 3.50 x 10^-1 4.48 x 10^31 4.45 x 10^-3 6.58 x 10^-2

Solved • Jul 1, 2019

Arrhenius Equation

Q. The rate constant for the decomposition of acetaldehyde, CH3CHO, to methane, CH4, and carbon monoxide, CO, in the gas phase is 1.74 110-2 L/mol/s at 713 K and 5.59 L/mol/s at 8G9 K. Determine the activation energy (in kJ/mol) for this decomposition

Solved • Jul 1, 2019

Arrhenius Equation

Q. How would a higher activation energy affect the rate of a reaction? The higher the activation energy, the ____ the reaction rate

Solved • Jul 1, 2019

Arrhenius Equation

Q. Question 18 A reaction is found to have an activation energy of 108 kj/mol if the rate constant for this reaction is 4.60x10-6 s-1 at 275K what is the rate constant at 366k

Solved • Jun 27, 2019

Arrhenius Equation

Q. 11) For the reaction: 2N2O5(g) →4NO2(g) +O2(g) the rate law is: Δ[O2] Δt =k[N2O5] At 300 K, the half-life is 2.50 × 104 seconds and the activation energy is 103.3 kJ/mol O2. What is the halflife at 310 K? A) 9.51 × 104 s B) 9.51 × 106 s C) 1.87× 10-1 s D) 6.57 × 103 s E) 2.49 × 104 s

Solved • Jun 26, 2019