For a certain reaction the specific rate constant, k, is 1.50 x 10-3 L mol-1 s-1 at 27 °C and 1.50 L mol-1 s-1 at 127 °C. For this reaction, the pre-exponential factor, A, in the Arrhenius equation has the value
8.3 x 103 L mol-1 s-1
1.5 x 10-3 L mol-1 s-1
9.7 kJ mol-1
1.5 x 106 kJ mol-1
1.5 x 109 L mol-1 s-1
For a certain reaction the specific rate constant, k, is 1.50 x 10-3 L mol-1 s-1...
For a certain reaction the specific rate constant, k, is 1.50 x 10-3 L mol-1 s-1 at 27 °C and 1.50 L mol-1 s-1 at 127 °C. For this reaction, the pre-exponential factor, A, in the Arrhenius equation has the value A. 8.3 x 103 L mol-1 s-1 B. 1.5 x 109 L mol-1 s-1 C. 1.5 x 106 kJ mol-1 D. 9.7 kJ mol-1 E. 1.5 x 10-3 L mol-1 s-1
For a certain reaction the specific rate constant, k, is 1.50 x 10-3 L mol-1 s-1 at 27 °C and 1.50 L mol-1 s-1 at 127 °C. For this reaction, the pre-exponential factor, A, in the Arrhenius equation has the value
The activation energy for a reaction is 15 kJ mol-1 at 27° C. A catalyst lowers the activation energy to 10 kJ mol at the same temperature. By what factor is the reaction rate increased? Assume that the reactant concentrations and the pre-exponential factor in the Arrhenius equation are unchanged. O A. 1.5 OB. 1.1 OC. 0.67 O D.7.4 O E. 1.7 x 107 Reset Selection
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...
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E, = 31.0 kJ/mol. If the rate constant of this - 1 - 1 reaction is 1.3 x 10° M S at 286.0 °C, what will the rate constant be at 192.0 °C? Round your answer to 2 significant digits. k = | M-1.5-1 x 6 ?
Variation of the rate constant with temperature for the first-order reaction 2N2(g) + O(g) → 2N2O4(g) is given in the following table. Determine the activation energy and pre-exponential factor for the reaction. What would be the rate constant at 350 K? Temperature / K Rate Constant / s-1 273 7.87 x 103 298 3.46 x 105 318 4.98 x 106 338 4.87 x 107 What is the activation energy in kJ/mol? Do not enter the units with your answer. What...
1. The rate constant for a certain reaction is k = 7.10×10−3 s−1 . If the initial reactant concentration was 0.350 mol L−1, what will the concentration be after 19.0 minutes? 2. A zero-order reaction has a constant rate of 3.70×10−4 mol L−1 s−1. If after 40.0 seconds the concentration has dropped to 9.00×10−2 mol L−1, what was the initial concentration?
E 12.0 kJ/mol. If the rate constant of this The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy sat 314.0 "C, what will the rate constant be at 347.0 °C reaction is 8.6x 10 M Round your answer to 2 signifcant digits. -0A X
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E = 56.0 kJ/mol. If the rate constant of this 3 - 1 - reaction is 2.7 x 10 M isat 252.0 °C, what will the rate constant be at 274.0 °C? Round your answer to 2 significant digits. -1 k = ï m-. 1 x s ?
R R=8.314 JK Imola 0%=273.15k (vi) Determine whether a precipitate of AgCl(s) will form on mixing 50.0 mL of 1.0 x 10-4 mol L-- Naci with 50.0 mL of 1.0 x 10-6 mol L-1 AgNO3. The Ksp for AgCl(s) is 1.8 x 10-10. (vii) A certain reaction is first order, and after 540 s after initiation of the reaction, 32.5 % of the reactant remains. What is the rate constant for this reaction? (viii) At 552.3 K, the rate constant...