The reaction F2 + 2CIO2 → 2FCIO2 was shown to give the following results at 250 K: Exp [F2]/mol [CIO;]/mol Rate of disappearance of F/mol dm s' 1.2 x 10 4.8 x 10 2.4 x 10 17. dm dm3 0.10 0.01 0.04 0.10 0.20 2 3 0.01 The reaction is A First order with respect to F2 and zero order with respect to CIO2 B Second order with respect to CIO, and first order with respect to F2 C First order with respect to F2 and first order with respect to CIO2 D Second order with respect to F2 and first order with respect to CIO2

The reaction F2 + 2CIO2 → 2FCIO2 was shown to give the following results at 250 K: Exp [F2]/mol [CIO;]/mol Rate of disappearance of F/mol dm s' 1.2 x 10 4.8 x 10 2.4 x 10 17. dm dm3 0.10 0.01 0.04 0.10 0.20 2 3 0.01 The reaction is A First order with respect to F2 and zero order with respect to CIO2 B Second order with respect to CIO, and first order with respect to F2 C First order with respect to F2 and first order with respect to CIO2 D Second order with respect to F2 and first order with respect to CIO2

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...

See similar textbooks

Similar questions

The activation energy for a reaction is determined to be 389.9 kJ. The rate constant at 20.5ºC is equal to 4.06 x 10-6 s-1. What is the rate constant at 34.9ºC for the reaction? Report your answer to the tenths place and using scientific notation (e.g. 1.27 x 103 or -1.27 x 10-3) and do not include units
For the standard Michaelis-Menten (MM) model (See image)If the experimenter accidentally setups the reaction such that [S]0 is not much greater than [E]0, derive the initial velocity of product formation, V0.
Consider the reaction data. A products T (K) | k (s-1) 325 0.383 825 0.611 What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all values. X1 Yi = X2 = Y2 = Determine the rise, run, and slope of the line formed by these points. rise: run: slope: What is the activation energy of this reaction? Ea J/mol ? II
Label the reaction profiles below as exothermic or endothermic and use them to calculate the activation energy of the forward and reverse reactions and the value of AH for the reaction. This is a reaction of profile of an 250 exothermic/endothermic reaction 200 PE 150 (kJ) Eaf = ...... 100 Ea, = 50 AH = Reaction pathway 100 This is a reaction of profile of an 80 exothermic/endothermic reaction 60 PE (kJ) A+B 40 Ear = C+D 20 Ear = ΔΗ Progress of the reaction
Consider the reaction data. A-products T (K)& (s- 325 0.376 875 0.719 What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all values. yi = X2 = Determine the rise, run, and slope of the line formed by these points. rise: run: slope: What is the activation energy of this reaction? J/mol Ea =
The yeast in bread dough feeds on sugar to produce carbon dioxide. Why does the dough rise faster in a warmer area? O The activation energy has been increased. O There are a greater number of effective collisions among reacting molecules at the higher temperature than at the lower temperature. O Atmospheric pressure decreases with increasing temperature.
reaction. assume k = 1. 2. At 25°C, k=1.55dm°mol-²min-l at an ionic strength of 0.0241 for a reaction in which the rate-determining step involves the encounter of two singly charged cations. Use the Debye-Huckel limiting law to estimate the rate constant at zero ionic strength. 3. The gas-phase reaction between F2 and IF, is first order in each of the reactants. The
1. The following data was obtained from decomposition of nitrogen oxide (NO). 2HX H2 + X2 T(K) 703 733 759 791 811 836 865 k (L mol-¹s-¹) Find; 0.011 0.035 0.105 0.343 0.790 2.14 4.95 (a) The activation energy, Ea. (b) The Arrhenius constant, A (c) The collision frequency, ZAA (d) The following mechanism was suggested for the reaction. Is the mechanism meet with the order of reaction? X₂ = X + X X + H2 H + XH + HX2 X + H₂ Fast Slow Fast
Please highlight the answers you found or underline them
Using collision theory, estimate the collision number for 1 mol of HI present in a volume of1 m3 at 300 K. Use dAA = 350 pm. If the activation energy for the decomposition of HI is 184 kJmol–1, what rate constant does kinetic theory predict at 300°C? To what pre-exponential factorand entropy of activation does this result correspond?