1
answer
0
watching
696
views
17 Nov 2019
Arrhenius equation can be represented as lnk = -E_a/(RT) + lnA where k is the rate constant, E_a the activation energy, T the absolute temperature, R the gas constant (8.314 J/molK), and A the collision frequency factor among molecules. Plotting of the set of data between Ink and 1/T reveals a straight line with its slope being E_a/R. Therefore, the activation energy, E_a, can be obtained because Excel plotting will give you the value for the slope and the gas constant R is already known. The following table is assumed to show the rate constants for the above reaction: Using these data, calculate the activation energy for the reaction. Show both the regenerated data table and the plot from which you obtain the activation energy. What is the value of the rate constant at 430.0 K? In (k_1/k_2) = E_a/R(1/T_2 - 1/T_1)
Arrhenius equation can be represented as lnk = -E_a/(RT) + lnA where k is the rate constant, E_a the activation energy, T the absolute temperature, R the gas constant (8.314 J/molK), and A the collision frequency factor among molecules. Plotting of the set of data between Ink and 1/T reveals a straight line with its slope being E_a/R. Therefore, the activation energy, E_a, can be obtained because Excel plotting will give you the value for the slope and the gas constant R is already known. The following table is assumed to show the rate constants for the above reaction: Using these data, calculate the activation energy for the reaction. Show both the regenerated data table and the plot from which you obtain the activation energy. What is the value of the rate constant at 430.0 K? In (k_1/k_2) = E_a/R(1/T_2 - 1/T_1)
Reid WolffLv2
18 Jan 2019