Given the following mechanism: 2NO N202 step 1 (fast, call the rate constants k1 and k-1) N202+H2N20 + H20 (slow, call the rate constant for this step k2) step 2 (call the rate constant for this step ka) N20 H2 N2 H20 step 3 Determine the overall reaction. а. b. Are there any intermediates in this reaction mechanism? If so, which one(s)? Determine the rate law. Intermediates may not appear in rate laws. Use the equilibrium с. expression to write the rate law only in terms of [reactants]. What is the overall order of the reactions? d. What is the molecularity of the rate determining step? е.

Given the following mechanism: 2NO N202 step 1 (fast, call the rate constants k1 and k-1) N202+H2N20 + H20 (slow, call the rate constant for this step k2) step 2 (call the rate constant for this step ka) N20 H2 N2 H20 step 3 Determine the overall reaction. а. b. Are there any intermediates in this reaction mechanism? If so, which one(s)? Determine the rate law. Intermediates may not appear in rate laws. Use the equilibrium с. expression to write the rate law only in terms of [reactants]. What is the overall order of the reactions? d. What is the molecularity of the rate determining step? е.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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10. Which mechanism is going to produce a faster reaction? Explain. Mechanism 2 Mechanism 1 STEP 1 NO + 03 → NO2 + 02 STEP 1 STEP 2 03 02 +0 03 +0 202 STEP 2 - 02 +0 NO2 +0 NO + 02 03 STEP 3 OVERALL 203 → 302 OVERALL 203 → 302
Analyze the following reaction mechanism: H2O + O → CIÓ + CF2CI CI + 202 4. Cl + CF2CI –→ CF2CI2 1. H2O2 2. O + CF2CI2 3. CIO + Oз -> Identify the reaction intermediates in this reaction. A) O, CIO, CI B) CI, CF;CI, CF2CI2 C) O, CIO, O, H20 D) O, CIO, CI, CF2CI E) O, CIO, CI, CF;CI2
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If the rate is given as -A[O2]/AT for a reaction, for the following reaction, what is the same rate given in terms of [H2O]? 2H2(g) + O2(g) – 2H20(g) A A[H20]/At B 24[H2O]/At c) -24[H20]/At D) A[H20]/2At
2 H₂ NO H₂O 2 H₂0 The reactants in the overall reaction are (include their correct coefficients): 2 NO 2 N₂0 N₂ N₂0 H₂ 2 N₂0₂ 2 N₂ Consider the following proposed reaction mechanism: N₂02 Step 1: NO + NO N202 Step 2: N202 + H2 - N2O + H20 Step 3: N2O + H2-N2 + H2O The second step is the slow (rate-determining) step. Answer the following questions: What is the correct rate law for the overall reaction? O rate = K[NO]²[H₂1² rate = k[NO]²[H₂] O rate= K[N₂0₂][H₂] rate = K[N₂0₂]²[H₂] The products in the overall reaction are (include their correct coefficients): N₂ NO 2 H₂O H₂ U U U U 2 H₂ 2 N₂0 N₂02 2 NO N₂0 H₂O 2 N₂02 2 N₂ The intermediates in the mechanism are: N₂0 H₂O NO N₂ N₂0₂ H₂
What would happen to the rate of a reaction with rate law rate = k[NO]<[H,] if the concentration of H, were halved? O A. The rate would not change. O B. The rate would be doubled. O C. The rate would be four times larger. O D. The rate would also be halved.
The rate law of the following reaction is : CH.CH-Br+ OH → CHCH-CH+Br A. Rate= k[CH,CH,-Br] B. Rate = k(CHCH-Br][OH] C. Rate = k(OH] D. Rate= kCHCH-Br][OHT %3D O D
Consider the reaction 2NH3(g) → N2(g) + 3H2(g) What is the rate of NH3 ? O ANH31/At -½ A[NH3]/At % A[NH31/2At 2 A[NH3]/At
Energy (kJ/mol) Select the most appropriate reaction coordinate diagram for this reaction from the graphs shown below: Energy (kJ/mol) 10 a Ob C d 15 20 A Energy (kJ/mol) 25 B 20 15 10 0 0 Reaction Coordinate Reaction Coordinate 25 20 C 15 16 14 10 Energy (kJ/mol) D 12 10 0 Reaction Coordinate Reaction Coordinate The reason that this graph is the best choice is the highest rate constant goes with the second step and the reaction is exothermic the highest rate constant goes with the first step and the reaction is endothermic the highest rate constant goes with the first step and the reaction is exothermic the highest rate constant goes with the second step and the reaction is endothermic In order to speed up the reaction, the team should decrease the temperature of the soap solution increase the temperature of the soap solution keep the temperature of the soap solution the same because the reaction is endothermic the reaction is exothermic the hydrogen peroxide molecules will have…