The rate constant for the reaction of Br2 with O3 to produce BrO and O2 is 5.9x10-13 at 238 K. At 258 K the rate constant is 7.7x10-13. What is the activation energy for this reaction?
The rate constant for the reaction of Br2 with O3 to produce BrO and O2 is...
12 Question (9 points) The rate constant for the reaction Br(g) +0,(8) - BrO(g) + (8) was determined at the four temperatures shown in the table below. T(K) 238 258 278 298 k (cm/moleculeos) 5.90 x 10-13 7.70 x 10-13 9.60 x 10-13 1.20 x 10-12 1st attempt I See Periodic Tab Plot the above data, and then use that data to calculate the activation energy for this reaction.
Reaction A $$O3(g)+Cl(g)ClO(g)+O2(g) $$A=2.93×10−11 cm3molecule • s and Ea=2.16 kJmol Reaction B $$O3(g)+NO(g)NO2(g)+O2(g) $$A=2.34×10−12 cm3molecule • s Ea=11.6 kJmol On the basis of the frequency factors and activation energy values above, calculate the rate constant for Reaction A at 298 K. On the basis of the frequency factors and activation energy values above, calculate the rate constant for Reaction B at 298 K. We were unable to transcribe this imageWe were unable to transcribe this image
Identify the catalyst and intermediate in the following multi-step mechanism: step 1: Br+O3 -> BrO+ O2 step 2: BrO + O3 -> Br +2O2 a. There is no catalyst or intermediate in the above reaction b. Catalyst: O2 Intermediate: O3 c. Catalyst: BrO∙ Intermediate: Br∙ d. Catalyst: O3 Intermediate: O2 e. Catalyst: Br∙ Intermediate BrO
Predict the rate law for the reaction 2BrO(g)-> Br2 (g) +O2 (g) if the following conditions hold true: Use k to represent the rate constant and place brackets [ ] arounds the molecular or atomic formula to designate concentration. The rate triples when [BrO] triples. Part 2 When [BrO] is halved, the rate decreases by a factor of 4. Part 3 The rate is unchanged when [BrO] is tripled.
Ozone decomposes to form oxygen molecules and oxygen atoms, O3(g) ? O2(g) + O(g), in the upper atmosphere. The energy of activation for this reaction is 93.1 kJ/mol. At 600 K, the rate constant for this reaction is 3.37
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...
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...
The rate constant for the reaction of nitrogen monoxide and ozone as shown in the corresponding image, is 1.67 x 1010 M-1 s-1 at 325 K. The rate constant for the same reaction at 375 K is 2.79 x 1010 M-1 s-1 determine the activation energy of this reaction. A) 10.4 kJ B) 19.7 kJ C) 21.3 kJ D) 100.4 kJ O3(g) + NO(g) → O2(g) + NO2(g)
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is reported in units of sl. What is the overall order of the reaction? 2) The rate law for a reaction was reported as rate=k[A] [B][C] with molar concentrations in moles per cubic decimetre and time in seconds. What are the units of k? 3) The rate constant for the pseudo first-order acid- catalysed hydrolysis of glucose is 4.07' 10-s. Calculate the half-life for the...
The molar equilibrium constant, Kc, is 7.7x10-11at 25oC for the reaction: 2HBr(g) <--> H2(g)+ Br2(g) What is the gas-phase equilibrium constant, Kp, for the reaction: Br2(g)+ H2(g) <--> 2HBr(g) a. 1.8x10-9 b. 7.7x10-11 c. 0.0 d. 1.3x1010 e. 3.8x1011