- The balanced equation for the reaction of nitrogen dioxide and fluorine is given below: 2...
The balanced equation for the reaction of nitrogen dioxide and fluorine is given below: 2 NO2 + F2 → 2 NO2F The proposed mechanism is: step 1: NO2 + F2 → NO2F + F (slow) step 2: F + NO2 → NO2F (fast) Based on this information, the following observations are made: I. The mechanism supports an experimentally determined rate law of rate = k[NO2]2[F2] II. F is an intermediate III. The reaction is first order in F2 Which of...
A mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is: step slow: F2+CIO, FCIO, + F step 2 fast: F+CIO, FCIO, (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank (3) Which species acts as a reaction intermediate? Enter formula....
1. Write a rate law from the image below: TRANSITION STATES Ea(step 2) Ea(step 1) slow fast Potential energy NO2F+ F+NO2 2NO2 + F2 REACTANTS ΔΗ 'nxn <0 2NO2F PRODUCT Reaction progress A. Rate = k [NO2] B. Rate = k [NO2][F2] C. Rate = k [NO212[F2] 2. What is the overall reaction? A. 2 NO2 + F2 → 2 NO2F B. NO2 + F2 → NO2F +F + NO2 C. NO2 + F2 → 2 NO2F 3. Write out...
A student proposed the following mechanism for the gas phase reaction of fluorine with chlorine dioxide. step 1 fast: 2 CIO, 2 C104 step 2 slow: C1204 +F2 ——2 FCIO2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. 20102 + F2 - 2FC10, + (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete...
6. The rate law for the following reaction is rate=k[NO2] (F2]: 2NO2(g) + F2(g) → 2NO2F(g) The mechanism proposed for this reaction is as follows: (i) NO2(g) + F2(g) → NO2F(g) + F(g) (ii) NO2(g) + F(g) → NO2F(g) Which elementary step is the rate-determining step in this reaction? Explain your answer in 1-2 sentences.
A student proposed the following mechanism for the gas phase reaction of fluorine with chlorine dioxide. step 1 fast: 2C10, C1,04 step 2 slow: Cl,04 + F2 — 2 FCIO2 (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall...
A mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is: step 1 slow: Fz+CIO, step 2 fast: F+CIO, FCIO, +F FCIO, (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula....
A) B) The following initial rate data are for the reaction of nitrogen dioxide with fluorine: 2 NO2 + F2 → 2 NO2F Experiment [F2), M [NO2], M 3.19 3.19 1.20 2.40 IllII Initial Rate, Ms-1 4.40x10-4 8.80x10-4 8.80x10-4 1.76x10-3 6.38 1.20 6.38 Complete the rate law for this reaction in the box below. Use the form k[A][B]" , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1...
1. Write a rate law from the image below: TRANSITION STATES Ea(step 2) Ea(step 1) slow fast Potential energy NO2F+ F+NO2 2NO2 + F2 REACTANTS ΔΗ 'nxn <0 2NO2F PRODUCT Reaction progress A. Rate = k [NO2] B. Rate = k [NO2][F2] C. Rate = k [NO212[F2]
The reaction between nitric oxide (nitrogen monoxide) and oxygen gives nitrogen dioxide according to the stoichiometric equation. 2 NO(g) 02(g)2 NO2(g) 1. Write the rate law expected if the reaction was found to occur in a single step The reaction is observed to be complex with the following mechanism is proposed: 2 NO N202 N202 2 NO N202 +02 → 2NO2 k2 kı k. -1 2. Use the steady state approximation to obtain the expression for the formation of NO2....