Rate of the reaction is the speed at which reactants are converted into products
19. For the reaction 2NO + O2 + 2NO2 the following reaction mechanism have been suggested;...
- For the reaction 2NO + O2 + 2NO the following reaction mechanism have been suggested; steps: NO + NON2O2 Fast step 2: N2O2 + O2 k2 2NO Slow and the apparent rate law was found to be R = kerr [NO] What would be the estimated effective activation energy, El. value, if the activation energies for forward and backward reactions in step 1 are 82 kJ mol" and 205 kJ moll, respectively, and the activation energy of step 2...
9. The reaction 2NO +O2 → 2NO2 is believed to occur by the following mechanism: 2NO ↔ N2O2 N2O2 + O2 → 2 NO2 a. Assume N2O2 to be in a steady state and derive the rate equation for the overall reaction. b. Under what condition does the rate equation reduce to second order kinetics in NO and first order kinetics in O2 at the same time?
Question 6: Reaction Mechanisms (9 points) For the reaction: 2NO2 → 2NO + O2 Suppose there are two possible mechanisms to define a particular reaction. These two mechanisms are proposed below: 1. NO2 → NO + O (slow) O + NO2 → O2 + NO (fast) 2. 2NO2 → NO3 + NO (slow) NO3 → NO + O2 (fast) a) Identify the rate for each reaction and the order of each reaction. (4 points) b.) Identify the intermediate for each...
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...
QUESTION 19 A proposed mechanism for the reaction 2NO(g) +2H2(g) → N2(g) + 2H2O(g): Step 1: 2NO(g) + N2O2(g) (very fast, reversible) Step 2: N2O2(g) + H2(g) → N2O(g) + H2O(g) (slow) Step 3: N2O(g) + H2(g) →N2(g) + H2O(g) (fast) What is the rate law for the overall reaction? Ok[NO]1/2[H2] k[NO]2[H2] k[NO] [H2)2 k[N20][H2] k[NO]2
Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature K 400 1.9x10^7 425 2.5x10^6 465 1.6x10^5 515 8.8x10^3 600 2.0x10^2 Use the data to find ΔrS∘ΔrS∘ for the reaction. (answer in J K-1 mol-1) The answer is NOT 158
For the reaction 2NO(g) + O2(g) ® 2NO2(g), DH° = -113.1 kJ/mol and DS° = -145.3 J/K·mol. Under which temperature conditions would the reaction be spontaneous? _________. a. For all temperatures b. Only at high temperatures c. Only at low temperatures
Given the reaction and following data: 2NO + O2 → 2NO2 Calculate the rate law constant and write the rate law. Trial [NO] (mol/L) [O2] (mol/L) Rate (mol/L/hr) 1 0.125 0.125 2.57 x 10-2 2 0.250 0.125 5.20 x 10-2 3 0.250 0.250 4.16 x 10-1
Consider the reaction: 2NO(g) + O2(g)2NO2(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.710 moles of NO(g) react at standard conditions. G°rxn = kJ
Calculate the enthalpy of the reaction 2NO(g) + O2(g) +2NO2 (g) given the following reactions and enthalpies of formation: 1;N, (g) +0,(g)NO,(g), AH = 33.2 kJ 2 N2(g) + O2(g) →NO(g), AHg = 90.2 kJ Express your answer with the appropriate units. View Available Hint(s) AH'- Value Units Submit