Subject :-- Chemistry Consider this initial rate data at a certain temperature in the table for the reactionOCI (aq) + (aq)Determine the rate law.k =rate = kOH(aq)→OI¯(aq) + Cl¯(aq)[OH™][I]Answer Bank[1-]²[OCI]Trial1234[OCI lo(M)[I lo[OH lo(M)(M)0.00187 0.00187 0.5100.00187 0.003500.5100.00353 0.001870.6830.001870.003500.740[OH-]²[OCI]²Determine the value of the rate constant for this reaction and the correct units.UnitsInitial rates(M/s)0.0003610.0006760.0005100.000466

Let the rate law equation for the given reaction is: rate=kOCl-xI-yOH-z ......(1) Where x is the…

Consider this initial rate data at a certain temperature in the table for the reaction OCI (aq) + (aq) Determine the rate law. rate = k OH(aq) →OI¯(aq) + Cl¯(aq) [OH™] [I] Answer Bank [1-]² [OCI] Trial 1 2 3 4 [OCI lo (M) 0.00187 0.00187 0.00350 0.00353 0.00187 0.00187 0.00350 [OH-]² [I lo [OH lo (M) (M) 0.00187 0.510 0.510 0.683 0.740 [OCI-]² Initial rates (M/s) 0.000361 0.000676 0.000510 0.000466

Consider this initial rate data at a certain temperature in the table for the reaction OCI (aq) + (aq) Determine the rate law. rate = k OH(aq) →OI¯(aq) + Cl¯(aq) [OH™] [I] Answer Bank [1-]² [OCI] Trial 1 2 3 4 [OCI lo (M) 0.00187 0.00187 0.00350 0.00353 0.00187 0.00187 0.00350 [OH-]² [I lo [OH lo (M) (M) 0.00187 0.510 0.510 0.683 0.740 [OCI-]² Initial rates (M/s) 0.000361 0.000676 0.000510 0.000466

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

See similar textbooks

Similar questions

Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
List at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.
. explain the difference between elementary reactions and multistep reactions.
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
Some bacteria are resistant to the antibiotic penicillin because they produce penicillinase, an enzyme with a molecular weight of 3104 g/mol that converts penicillin into inactive molecules. Although the kinetics of enzyme-catalyzed reactions can be complex, at low concentrations this reaction can be described by a rate equation that is first order in the catalyst (penicillinase) and that also involves the concentration of penicillin. From the following data: 1.0 L of a solution containing 0.15 g ( 0.15106 g) of penicillinase, determine the order of the reaction with respect to penicillin and the value of the rate constant. [Penicillin] (M) Rate (mol/L/min) 2.0106 1.01010 3.0106 1.51010 4.0106 2.01010
The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.
One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a catalyst? b. Which species is an intermediate? c. Ea for the uncatalyzed reaction O3(g)+O(g)2O2(g) is 14.0 kJ. Ea. for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25C? Assume that the frequency factor A is the same for each reaction.
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
Consider the following energy diagram (not to scale) for the reaction. 2CH3(g)C2H6(g) (a) What is the activation energy of the forward reaction? (b) At what point would 2CH3 (g) appear? (c) What is H for the reaction? (d) What is the activation energy of the reverse reaction? (e) At what point would C2H6 certainly be found? (f) What is any species at point C called?