The rate constant for the reaction below was determined to be 3.241×10-5 s–1 at 800 K. The activation energy of the reaction is 255 kJ/mol. What would be the value of the rate constant at 9.10×102 K? N2O --> N2 + O
The rate constant for the reaction below was determined to be 3.241×10-5 s–1 at 800 K....
The rate constant for the reaction below was determined to be 3.241×10-5 s–1 at 800 K. The activation energy of the reaction is 265 kJ/mol. What would be the value of the rate constant at 9.60×102 K? $$N2O(g) N2(g)+O(g) (explain all steps and including calculator)
See HintSee Periodic Table The rate constant for the reaction below was determined to be 3.241×10-5 s–1 at 800 K. The activation energy of the reaction is 215 kJ/mol. What would be the value of the rate constant at 9.80×102 K? $$
The half-life for the reaction was determined to be 2.14 × 104 s at 800 K. The value of the half-life is independent of the inital concentration of N2O present. The activation energy of the reaction is 259.00 kJ/mol. N2O(g)->N2(g)+O(g) what would be the half life at 900.10K?
14 Question e See page 585 (1 point) 1st attempt See Periodic Table See Hint -5 -1 The rate constant for the reaction below was determined to be 3.241x10 s a 225 kJ/mol. What wou Id be the value of the rate constant at 9.40x10 K? N20(g) > N2 (8) +O (g) 800 K. The activation energy of the reaction is -1 14 Question e See page 585 (1 point) 1st attempt See Periodic Table See Hint -5 -1 The...
The half-life for the reaction below was determined to be 2.14 x 104 s at 800 K. The value of the half-life is independent of the inital concentration of N20 present. The activation energy of the reaction is 226.00 kJ/mol N20(g)N2(8) +0(g) 4th attempt See Periodic Table See Hint What would be the half-life at 1050.43 K? 33.3 The half-life for the reaction below was determined to be 2.14 x 104 s at 800 K. The value of the half-life...
The half-life for the reaction below was determined to be 2.14 x 10's at 800 K. The value of the half-life is independent of the inital concentration of N20 present. The activation energy of the reaction is 259.00 kJ/mol. NO(g) - Nag) +0g) 1st attempt See Periodic Table See Hint What would be the half-life at 1000.32 K?
A reaction has a rate constant of 0.0177 s-1 at 400.0 K. If the reaction has activation energy of 125 kJ/mol, calculate the rate constant at 500.0 K.A reaction has a rate constant of 0.0177 s-1 at 400.0 K. If the reaction has activation energy of 125 kJ/mol, calculate the rate constant at 500.0 K.
The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 35 × 10⁻⁴ s⁻¹ at 322 K, what is the rate constant at 273 K? An experimental plot of ln(k) vs. 1/T is obtained in lab for a reaction. The slope of the best-fit line for the graph is -3090 K. What is the value of the activation energy for the reaction in kJ/mol?
If a first-order reaction has a rate constant of 2.11 x 10-1 s-1 at a temperature of 22.3°C, what would the value of k be if the reaction temperature has changed to 43.4 °C given the activation energy is 52.9 kJ/mol?
Part A: The rate constant for a certain reaction is k = 1.90×10−3 s−1 . If the initial reactant concentration was 0.150 M, what will the concentration be after 7.00 minutes? Part B: A zero-order reaction has a constant rate of 4.60×10−4 M/s. If after 30.0 seconds the concentration has dropped to 8.00×10−2 M, what was the initial concentration? Part C: A certain reaction has an activation energy of 60.0 kJ/mol and a frequency factor of A1 = 7.80×1012 M−1s−1...