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Use the generic elementary steps shown to below to answer the following questions. A + BC...
8) A reaction occurs via the following sequence of elementary steps. What is the rate law based on this reaction mechanism? very fast slow fast 1st step: A B 2nd step: B+C D 3rd step: D - 2E A) rate = k[E]2 B) rate = k[A] [C] C) rate = k[B][C] D) rate = k[D] E) rate = k[A] [B]
3. Use the proposed reaction mechanism to answer the following questions; Elementary 1: 2NO2Cl <---> ClO2 + N2O + ClO Elementary 2: N2O + ClO2 <---> NO2 + NOCl Elementary 3: NOCl + ClO ---> NO2 + Cl2 a) What is the overall (reduced) reaction? b) Identify any intermediates. c) Determine the rate law expression for each elementary reaction. (fast) (fast) (slow)
What two criteria must a plausible mechanism meet? Select both criteria in the options. elementary steps must sum to the net reaction the mechanism must include at least two intermediates the slow step must always be the first step in the mechanism the rate law of the net reaction must match the rate law of the slowest step the mechanism must involve at least one catalyst Areaction profile is shown. Which step is the rate limiting (or rate determining) step...
21. A reaction proceeds by a series of elementary steps as shown below. The activation energy and heat of reaction are shown for each step. Step No. Elementary step Activation energy Enthalpy of reaction A + B2 → AB, 4 kJ/mol -10 kJ/mol 2 AB2+ C → ABC + BC 30 kJ/mol +5.2 kJ/mol 3 ABC + B2 → AB + BC 10 kJ/mol -7.8 kJ/mol a) What is the overall equation for this reaction? (1 mark) b) What is...
A reaction mechanism is defined as the sequence of reaction steps that define the pathway from reactants to products. Each step in a mechanism is an elementary reaction, which describes a single molecular event of usually one or two molecules interacting. The rate law for an overall reaction is the rate law for the slowest step in the mechanism, which is directly related to the stoichiometric coefficients of the reactants. The exception to this rule occurs when the slowest step...
Consider the following 2 - step reaction A + B2 + C → AB + BC (slow) A + BC → AB + C (fast) which of the following statements is/are correct? 1. The rate law is third order. 2. BC is a reaction intermediate. 3. C is a catalyst. A. none B. 2 & 3 only C. 1 & 2 only D. 1 & 3 only E. all
8. (2 points) Consider the mechanism below Step 1 (slow) A2 BC AB+AC AB BC B2AC Step 2 (fast) B2+ 2 AC overall A22 BC What is the rate law of the reaction? a. b. What compound is considered an intermediate?
this is all that is given 21. A reaction proceeds by a series of elementary steps as shown below. The activation energy and heat of reaction are shown for each step. Step No. Activation energy Elementary step A + B → AB Enthalpy of reaction 4 kJ/mol -10 kJ/mol AB + C → ABC + BC 30 kJ/mol +5.2 kJ/mol ABC + B → AB + BC 10 kJ/mol -7.8 kJ/mol a) What is the overall equation for this reaction?...
Seat # Ver. K J. Quest. 6 (9 pts). The following initial rates were obtained for the reaction -120 kJ Δ Η 2C 2A +B [B] (M) 0.30 0.60 [A] (M) 0.20 Rate (M/s) 0.127 0.40 1.02 0.254 0.509 0.60 0.20 0.40 0.30 a. Determine the rate law for the reaction. b. Calculate the rate when B 0.40 M and A 0.65 M. a. With the aid of the rate law, propose a plausible two-step mechanism for the reaction. Label...
Sketch a reaction coordinate energy diagram for the following elementary steps, which describe an endothermic reaction. Write the overall rate law for this process. What is the reaction order? A+B=3C. fastest C+2D= . Slow E=F. Fast