Be sure to answer all parts. Archaeologists can determine the age of artifacts made of wood or bone by measuring the amount of the radioactive isotope 1"C present in the object. The amount of isotope decreases in a first-order process. If 22.2% of the original amount of 14C is present in a wooden tool at the time of analysis, what is the age of the tool? The half-life of 14C is 5,730 yr. Give your answer in scientific notation. 14, x 10 yr

Be sure to answer all parts. Archaeologists can determine the age of artifacts made of wood or bone by measuring the amount of the radioactive isotope 1"C present in the object. The amount of isotope decreases in a first-order process. If 22.2% of the original amount of 14C is present in a wooden tool at the time of analysis, what is the age of the tool? The half-life of 14C is 5,730 yr. Give your answer in scientific notation. 14, x 10 yr

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 13.51QE: The half-life of tritium, 3H, is 12.26 years. Tritium is the radioactive isotope of hydrogen. (a)...

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Iodine-131 is used to treat tumors in the thyroid. Its decomposition is first-order with a half-life of 8.1 days. If a patient is given a sample containing 5.00 mg of I-131, how long will it take for 32% of the isotope to remain in her system?
The half-life of tritium, 3H, is 12.26 years. Tritium is the radioactive isotope of hydrogen. (a) What is the rate constant for the radioactive decay of tritium, in y1 and s1? (b) What percentage of the original tritium is left after 61.3 years?
Sucrose, a sugar, decomposes in acid solution to give glucose and fructose. The reaction is first-order in sucrose, and the rate constant at 25 C is k = 0.21 h1. If the initial concentration of sucrose is 0.010 mol/L, what is its concentration after 5.0 h?
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay: HCOOH(g)CO2(g)+H2(g) The rate of reaction is monitored by measuring the total pressure in the reaction container. Time (s) Pressure (torr) 0 220 50 324 100 379 150 408 200 423 250 431 300 435 Calculate the rate constant and half-life in seconds for the reaction. At the start of the reaction (time = 0), only formic acid is present. (HINT: Find the partial pressure of formic acid using Dalton's law of partial pressure and the reaction stoichiometry to find PHCOOH at each time.)
Hydrogen peroxide and the iodide ion react in acidic solution as follows: H2O2(aq)+3I(aq)+2H+(aq)I3(aq)+2H2O(l) The kinetics of this reaction were studied by following the decay of the concentration of H2O2 and constructing plots of ln[H2O2] versus time. All the plots were linear and all solutions had [H2O2]0 = 8.0 104 mol/L. The slopes of these straight lines depended on the initial concentrations of I and H+. The results follow: [I]0 (mol/L) [H+]0 (mol/L) Slope (min1) 0.1000 0.0400 0.120 0.3000 0.0400 0.360 0.4000 0.0400 0.480 0.0750 0.0200 0.0760 0.0750 0.0800 0.118 0.0750 0.1600 0.174 The rate law for this reaction has the form Rate=[H2O2]t=(k1+k2[H+])[I]m[H2O2]n a. Specify the order of this reaction with respect to [H2O2] and [I]. b. Calculate the values of the rate constants, k1 and k2. c. What reason could there be for the two-term dependence of the rate on [H+]?
The decomposition of many substances on the surface of a heterogeneous catalyst shows the following behavior: How do you account for the rate law changing from first order to zero order in the concentration of reactant?
In the presence of excess thiocyanate ion, SCN, the following reaction is first order in iron(III) ion, Fe3+; the rate constant is 1.27/s. Fe3+(aq)+SCN(aq)Fe(SCN)2+(aq) What is the half-life in seconds? How many seconds would be required for the initial concentration of Fe3+ to decrease to each of the following values: 25.0% left, 12.5% left, 6.25% left, 3.125% left? What is the relationship between these times and the half-life?
Explain why half-lives are not normally used to describe reactions other than first order.