For a different reaction, K. = 103, kg = 6.76 x 10's1, and k, = 65.7 s. Adding a catalyst increases the forward rate constant to 9.73x105 s-1. What is the new value of the reverse reaction constant, k, after adding catalyst? Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M between each measurement. •s1 include - (multiplication dot) > View Available Hint(s) HA k, = Value s 1

For a different reaction, K. = 103, kg = 6.76 x 10's1, and k, = 65.7 s. Adding a catalyst increases the forward rate constant to 9.73x105 s-1. What is the new value of the reverse reaction constant, k, after adding catalyst? Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M between each measurement. •s1 include - (multiplication dot) > View Available Hint(s) HA k, = Value s 1

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

At 40^0c, H202 (aq) will decompose according to the foll. reaction: 2 H202 (aq) ----2H20(l) +02 (g) The foll. data were collected for the concentration of h202 at various times. Time. [H202] (mol/L) 0. 1.600 3.10*10^4 0.592 6.20*10^4. 0.219 (a) Calculate the average rate of decomposition in H202 between0 and 3.10 * 10^4 s. use this rate to calculate the average rate of production 02 (g) over the same time period. (b) What are these rates for the time period 3.10*10^4 s. to 6.20 *10^4 s.? Rate of H202 decomposition Rate of O2 Production
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
3. Draw a reaction energy diagram, and label the product (P), reactant (R), transition states (TS1, TS2, etc.), intermediates (INT1, INT2, etc.) and activation energies (AG‡₁, AG 2, etc.) for a reaction with the following criteria: i. A three-step, endothermic reaction; ii. AG3 > 0 but AG₁ AG‡₁ >> AG‡₂. Which species does the structure of the transition state of the rate-determining step resemble?
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 =
Calculate the reaction rate for each trial using an average of the time (in sec) for each trial
Consider a reaction taking place at two different temperatures, T₁= 50 K and T₂- 150 K. What is the mathematical expression showing at which temperature the reaction will be faster?
Help, please answer my chemistry question ASAP! It is attached below
Captain Marvelibrium discovered a figure with data frorh an experiment left by Le Châtelier Flipdime. Consider the following data where A andB are mixed at initial concentrations indicated. Upon reacting the concentrations change a can be read from the plot. The reaction is A(g) + B(g) = C(g). C Time (s) Based on figure, calculate the value for Ke for the reaction. Submit Answer Tries 0/99 This discussion is closed. Send Feedback MAR 10 étv МacВос Air 000 esc F1 F2 F3 F4 F5 F6 #3 $4 3. 4 CO AB 3. Concentration (mol.dm-3)
If a catalyst is added, what direction would the equilibrium position shift to?
Consider this graph of concentration versus time. Concentration (M) V 1.00 0.84 0.52 0.32 0.00 1st attempt Part 1 X - + Time log B₂ A₂ A3B What is the mass action expression for the reaction? Do not add multiplication symbols or spaces to your answer. Feedback cos. 8 See Periodic Table See Hint