Calculate the activation energy in kJ/mol for the following iodine clock reaction using the information give below. Recordthe answer for 2 decimal places.S,0, na + 21'ag)......> 2 SO, ao) + I2lag)Rate = k[S2O] (I-] (kis the rate constant)%3DRate =(t is the time recorded for the reaction)2xtR= 8.314 J K mol1Temperature Volume of 0.20Volume of Volume of 0,01 Volume ofTime°C)M S,0,20.20M IM S20,?DI water(s)22.02.0 mL5.0 ml2.0 ml1.0 ml6540,02.0 mL5.0 ml2.0 ml1.0 ml8.

We are given experimental data for two different temperature values. The activation energy can be…

Calculate the activation energy in kJ/mol for the following iodine clock reaction using the information give below. Record the answer for 2 decimal places. S,0, ) + 21'ag) - 2 So, ) + Iza) Rate = k[S,0* (I-1 (kis the rate constant) (5,0) 2xt Rate = (t is the time recorded for the reaction) R- 8.314 J K mol1 Temperature Volume of 0.20 M S,0, Volume of Volume of 0.01 Volume of Time 0.20M I M S,0, DI water (s) 22.0 2.0 ml 5.0 ml 2.0 ml 1.0 mL 65 40.0 2.0 ml 5.0 ml 2.0 ml 1.0 ml

Calculate the activation energy in kJ/mol for the following iodine clock reaction using the information give below. Record the answer for 2 decimal places. S,0, ) + 21'ag) - 2 So, ) + Iza) Rate = k[S,0* (I-1 (kis the rate constant) (5,0) 2xt Rate = (t is the time recorded for the reaction) R- 8.314 J K mol1 Temperature Volume of 0.20 M S,0, Volume of Volume of 0.01 Volume of Time 0.20M I M S,0, DI water (s) 22.0 2.0 ml 5.0 ml 2.0 ml 1.0 mL 65 40.0 2.0 ml 5.0 ml 2.0 ml 1.0 ml

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.92QE

See similar textbooks

Similar questions

A substance undergoes first-order decomposition. After 40.0 min at 500°C, only 12.5% of the original sample remains. YYliat is the half-life of the decomposition? If the original sample weighed 243 g, how much would remain after 2.00 h?
If the activation energy of a reaction is 9.13 kJ, then what is the percent increase in the rate constant when the temperature is increased from 27C to 69C?
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?
The precipitation of egg albumin in water at 100C has an activation energy of 52.0 kJ/mol. By what percent does the rate of precipitation decrease if the water is at 92C?
Show how equation 20.33 reduces to a simpler form of an integrated first-order rate law when the reverse reaction of an equilibrium is negligible.
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay. HCOOH(g) CO2(g) + H2(g) At 550 C, the half-life of formic acid is 24.5 minutes. (a) What is the rate constant, and what are its units? (b) How many seconds are needed for formic acid, initially 0.15 M, to decrease to 0.015 M?
Suppose that the half-life of steroids taken by an athlete is 42 days. Assuming that the steroids biodegrade by a first-order process 5, how long would it take for 164 of the initial dose to remain in the athlete’s body?
The first-order rate constant for the decomposition of a certain hormone in water at 25C is 3.42104day1. (a) If a 0.0200 M solution of the hormone is stored at 25C for two months, what will its concentration be at the end of that period? (b) How long will it take for the concentration of the solution to drop from 0.0200 M to 0.00350 M? (c) What is the half-life of the hormone?
Compare the functions of homogeneous and heterogeneous catalysts.
The hypothetical reaction QR+Xproductswas monitored at 27C as a function of time. The following plots are obtained: (a) Write the rate expression for the reaction. (b) What is the rate constant if the rate of the reaction is 0.29 mol/L min when [ QR ]=[ X ]=1.000M? (c) What is the half-life for the consumption of QR when [ QR ]=0.0866M? (d) If the initial concentration of [ X ]=5.00M, what is [ X ] after 4.7 min?
Bacteria cause milk to go sour by generating lactic acid. Devise an experiment that could measure the activation energy for the production of lactic acid by bacteria in milk. Describe how your experiment will provide the information you need to determine this value. What assumptions must be made about this reaction?
What is the difference between average rate, initial rate, and instantaneous rate?