Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 25, Problem 73SCQ
Interpretation Introduction
Interpretation: To calculate the total number of fish in the lake.
Concept introduction:
The isotope dilution method is given as:
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Element
Atomic Number: 1
Name:
Hydrogen
Symbol:
H
Atomic Number
1
O'H
O2H
25
50
75
Atomic Number
An atom can be thought of as being
formed from a number of combined 'H
atoms with additional neutrons in the
nucleus. The mass of an atom is less
than that of the combined masses of
the nuclear particles from which it is
formed. This "mass loss" is an
indication of the stablity of the atom's
nucleus. In order to compare different
atoms, the relative mass loss (in g/mol)
is defined as:
[(number protons x mass of 'H)+(number of neutrons x mass of n)] - atomic mass
number of protons + number of neutrons
The atom's binding energy (the energy
associated with holding the nucleus
together) can be calculated as:
relative mass loss (kg/mol) x (2.998 x 10°m/s)
The resulting units are joules/mole.
Because calculating the relative mass
loss involves dividing by the total
number of nucleons (protons +
neutrons), the binding energy is called
the 'binding energy per nucleon.'
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Relative…
An archeologist was investigating a dig site and found charcoal in a pre-historic fire pit. Charcoal consists mostly of the element carbon. There are three naturally occurring isotopes of carbon: 12C, 13C, and 14C. Carbon-14 is radioactive and can be used to date the charcoal. The archeologist collected a sample for testing and learned that the carbon-14 activity was found to be 10 counts per minute. A sample of new charcoal of similar size showed a carbon-14 activity of 640 counts per minute.
How many carbon-14 half-lives have occurred?
Estimate the age of the charcoal. (The half-life of 14C is 5,730 years.)
NUCLEAR CHEMISTRY: Consider the nuclei 1150Sn. Determine its mass defect in kilograms if its atomic mass is 116.932 amu. The mass of a proton and neutron are 1.0073 and 1.0087 amu, respectively.
Express your answers in three decimal places in scientific notation, i.e., 6.022e23 to represent 6.022 x 1023 Do not include the unit.
Chapter 25 Solutions
Chemistry & Chemical Reactivity
Ch. 25.2 - Prob. 25.1CYUCh. 25.2 - Prob. 25.2CYUCh. 25.3 - Prob. 25.3CYUCh. 25.3 - Prob. 25.4CYUCh. 25.4 - Prob. 25.5CYUCh. 25.4 - Prob. 25.6CYUCh. 25.4 - Prob. 25.7CYUCh. 25.5 - Prob. 25.8CYUCh. 25.8 - Prob. 25.9CYUCh. 25.8 - Prob. 1.1ACP
Ch. 25.8 - Prob. 1.2ACPCh. 25.8 - Prob. 1.3ACPCh. 25.8 - Calculate the molar mass (atomic weight) of...Ch. 25.8 - Prob. 2.1ACPCh. 25.8 - Prob. 2.2ACPCh. 25.8 - Prob. 2.3ACPCh. 25.8 - Prob. 2.4ACPCh. 25.8 - Prob. 2.5ACPCh. 25.8 - Prob. 2.6ACPCh. 25.8 - Prob. 3.1ACPCh. 25.8 - Prob. 3.2ACPCh. 25.8 - Prob. 3.3ACPCh. 25.8 - Prob. 3.4ACPCh. 25 - Prob. 1PSCh. 25 - Prob. 2PSCh. 25 - Prob. 4PSCh. 25 - Prob. 5PSCh. 25 - Prob. 6PSCh. 25 - Prob. 7PSCh. 25 - Prob. 8PSCh. 25 - Prob. 9PSCh. 25 - Prob. 10PSCh. 25 - Prob. 11PSCh. 25 - Prob. 12PSCh. 25 - Prob. 13PSCh. 25 - Prob. 14PSCh. 25 - Prob. 15PSCh. 25 - Prob. 16PSCh. 25 - Prob. 17PSCh. 25 - Prob. 18PSCh. 25 - Prob. 19PSCh. 25 - Prob. 20PSCh. 25 - Prob. 21PSCh. 25 - Prob. 22PSCh. 25 - Prob. 23PSCh. 25 - Prob. 24PSCh. 25 - Prob. 25PSCh. 25 - Prob. 26PSCh. 25 - Prob. 27PSCh. 25 - Prob. 28PSCh. 25 - Prob. 29PSCh. 25 - Prob. 30PSCh. 25 - Prob. 31PSCh. 25 - Prob. 32PSCh. 25 - Prob. 33PSCh. 25 - Prob. 34PSCh. 25 - Prob. 35PSCh. 25 - Prob. 36PSCh. 25 - Prob. 37PSCh. 25 - Prob. 38PSCh. 25 - Prob. 39PSCh. 25 - Prob. 40PSCh. 25 - Prob. 41PSCh. 25 - Prob. 42PSCh. 25 - Prob. 43PSCh. 25 - Prob. 44PSCh. 25 - Prob. 45PSCh. 25 - Prob. 46PSCh. 25 - Prob. 47PSCh. 25 - Prob. 48PSCh. 25 - Prob. 49PSCh. 25 - Prob. 50PSCh. 25 - Prob. 51PSCh. 25 - Prob. 52PSCh. 25 - Prob. 53PSCh. 25 - Prob. 54PSCh. 25 - Prob. 55PSCh. 25 - Some of the reactions explored by Ernest...Ch. 25 - Prob. 57GQCh. 25 - Prob. 58GQCh. 25 - Prob. 59GQCh. 25 - Prob. 60GQCh. 25 - Prob. 61GQCh. 25 - Prob. 62GQCh. 25 - Prob. 63GQCh. 25 - Prob. 64GQCh. 25 - Prob. 65ILCh. 25 - Prob. 66ILCh. 25 - Prob. 67ILCh. 25 - Prob. 68ILCh. 25 - Prob. 69ILCh. 25 - Prob. 70ILCh. 25 - Prob. 71SCQCh. 25 - Prob. 72SCQCh. 25 - Prob. 73SCQCh. 25 - Prob. 74SCQCh. 25 - Prob. 76SCQCh. 25 - Prob. 77SCQCh. 25 - Prob. 78SCQCh. 25 - Prob. 79SCQ
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- 2.86 For some uses, the relative abundance of isotopes must be manipulated. For example, a medical technique called boron neutron capture therapy needs a higher fraction of 10B than occurs naturally to achieve its best efficiency. What would happen to the atomic weight of a sample of boron that had been enriched in 10B? Explain your answer in terms of the concept of a weighted average.arrow_forwardThe radioactive isotope strontium-81 is used in medical imaging as indicated on the table above. If 77.1 milligrams of strontium-81 is administered to a patient, how many milligrams are left in the body after 66.6 minutes?__ mgarrow_forwardFILL IN THE BLANK This experiment concerns kinetics and isotopes. Isotopes are atoms of an element that differ only in the number of (electrons, neutrons, protons?) We rarely talk about isotopes unless radioactivity is involved. A radioactive isotope can emit alpha rays which are (electrons, photons, helium 4 nuclei?) beta rays which are (electrons, photons, helium 4 nuclei?) or gamma rays which are (electrons, photons, helium 4 nuclei?) Despite our rare discussion of isotopes we actually cover them very early in our study of chemistry when we learn that the Periodic Table advertises the average atomic mass of an element as a weighted average of the various isotopes. Chlorine has two isotopes: chlorine-35 massing at about 35 g/mol and chlorine-37 massing at about 37 g/mol. The average atomic mass of chlorine is 35.453 g/mol instead of being close to 36 g/mol because (Cl-37, Cl-35?) is more abundant than the other isotope. The fact that the Periodic Table reports weighted average molar…arrow_forward
- The number of protons in the nuclide neptunium-237 Express your answer as an integer.arrow_forwardErnest Rutherford (the first New Zealander to be awarded the Nobel Prize in Chemistry) demonstrated that nuclei were very small and dense by scattering helium-4 nuclei (*He) from gold-197 nuclei (197AU). The energy of the incoming helium nucleus was 7.25 × 10¬13 J, and the masses of the helium and gold nuclei were 6.68 × 10¬27 kg and 3.29 x 10-25 kg, respectively (note that their mass ratio is 4 to 197. 3 J, Assume that the helium nucleus travels in the +x-direction before the collision.) (a) If a helium nucleus scatters to an angle of 132° during an elastic collision with a gold nucleus, calculate the helium nucleus' final speed (in m/s) and the final velocity (magnitude in m/s and direction counterclockwise from the +x-axis) of the gold nucleus. 120° He nucleus Gold nucleus 4He speed m/s 197 Au velocity m/s 197 Au direction ° counterclockwise from the +x-axİs (b) What is the final kinetic energy (in J) of the helium nucleus? Jarrow_forward8 1 is called the mass defect. Its interpretation can be found in Einstein's mass-energy eq formed, some of the mass of its constituent protons and the neutrons gets converted i the nucleus together. 16 The most common oxygen isotope is 0, but the rarer isotopes O and 0 of this element also exist in nature. These less common isotopes are stable, and measurements of their abundances have proved crucial in many fields of scientific research. For example, in climate research studies, the ratio of O to 0 measured in natural Part C 8. waters, as well as in polar ice, can provide useful information on the precipitiation history in a given area. This is because water containing O evaporates less readily, and condenses more easily as precipitation, than water containing 0. What is the equivalent energy EB of the mass defect of an atom of 0? 8 18 8 Express your answer in megaelectron volts to four significant figures. 16 View Available Hint(s) ΑΣφ ? EB = MeV Submit Previous Answersarrow_forward
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- Which of the following materials can neutrons pass through? Concrete Lead ☐ Water Metal ☐ Paperarrow_forwardDe All chan 1. Why is the neutron to proton ratio so important? It determines the stability of the nucleus based on the shielding effect of the neutrons. The neutron to proton ratio describes a radioactive element's half-life. Scientists made up this concept because they wanted to create radiation. An atom's nucleus likes to have the same number of neutrons and protons, so knowing that ratio is important. 00:53:35 PREVIOUS 1 of 20 NEXT SAVEarrow_forwardFill in the information missing from this table. nuclide protons neutrons Z A 0 0 0 66 164 0 70 106 0 0 0 0 38 18 Ar X Ś ?arrow_forward
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