Sulfur (S) has four naturally occuring isotopes, S-32, S-33, S-34, and S-36. Calculate the average atomic mass of sulfur. S-32 has an isotopic mass of 31.972 u and an abundance of 95.02%. S33 has an isotopic mass of 32.971 u and an abundance of 0.75%. S34 has an isotopic mass of 33.967 u and an abundance of 4.21%. S36 has an isotopic mass of 35.967 u and an abundance of 0.02%.

Sulfur (S) has four naturally occuring isotopes, S-32, S-33, S-34, and S-36. Calculate the average atomic mass of sulfur. S-32 has an isotopic mass of 31.972 u and an abundance of 95.02%. S33 has an isotopic mass of 32.971 u and an abundance of 0.75%. S34 has an isotopic mass of 33.967 u and an abundance of 4.21%. S36 has an isotopic mass of 35.967 u and an abundance of 0.02%.

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

For an unknown isotope ion, fill in the missing information below. Isotope symbol: (For the isotope symbol, type in without superscripts. For example, 184w4+ would be typed in as "184W4+" or "184 W 4+") Number of protons: 92 Number of neutrons: Number of electrons: 88 Mass number: 235 ns Charge:
An atom of chlorine (CI) has a mass number of 37. Given only this information, which of the following statements can you be absolutely sure is true? The atom of chlorine has 18 neutrons. The atom of chlorine has 37 neutrons. The atom of chlorine has 17 protons. The atom of chlorine has 17 electrons.
A new element has been discovered. This element has an atomic mass of 120.946 amu and only two naturally occurring isotopes. The first isotope has a natural abundance of 47.12% and an isotopic mass of 119.345 amu. What is the mass of the other isotope in amu?
Chlorine has two naturally occurring isotopes, 35Cl and 37Cl. What is the mass number of each? How many protons, neutrons, and electrons are present in each?
For an unknown isotope ion, fill in the missing information below. Isotope symbol: I (For the isotope symbol, type in without superscripts. For example, 184w4 would be typed in as "184W4+" or "184 W 4+") Number of protons: 92 Number of neutrons: 143 Number of electrons: 88 Mass number: 235 Charge: +4
Gallium has two naturally occurring isotopes, 69Ga and 71Ga. The average atomic mass of galllium is 69.70 amu. Which of the following statements concerning the relative abundance of each isotope is correct? a) The abundance of 71Ga is greater than 69Ga. b) The abundance of 71Ga is less than 69Ga. c) The abundance of 71Ga is exactly equal to the abundance of 69Ga. d) Based on the atomic mass, only 69Ga occurs naturally. e) Not enough data is provided to determine the correct answer.
A new element has been discovered with two isotopes having masses of 84.63 amu and 90.63 amu. The average mass is 88.01 amu. Write the isotopic atomic mass that is the most abundant.
Naturally occurring neon exists as three isotopes. 90.51% is Ne-20 with a mass of 19.99 amu, O.27% is Ne-21 with a mass of 20.99 amu, and9.22% is Ne-22 with a mass of 21.99 amu. What is the atomic mass of neon? O 20.18 amu O 62.97 amu O 10.00 amu O 20.99 amu
1- For each of the following atoms, calculate the number of protons and neutrons in the nucleus and the number of electrons outside the nucleus (assume neutral atoms). element number of number of number of electrons mass number (A) symbol 126C protons (Z) neutrons 12 10 12 10 14 27 10 23,1Na 11 17 18 2- Calculate the atomic mass to four significant figures for carbon, given the following data: Isotope Exact Atomic Mass (amu) 12.00000 13.00335 Abundance in Nature (%) 98.89 1.110 12C 13C
Calculated the weighted average of a substance from space. It has an abundance of 30.0% and 70.0% for its two isotopes. The atomic mass for the two isotopes are 111.653amu and 113.665amu, respectively.
Which of the following represents a pair of isotopes? Atomic Number | Mass Number 1. 6| 14 A II. 7| 14 1. 617 B II. 14 | 14 1. 6| 14 II. 14 | 28 I. 7 | 13 D II. 7 | 14 1. 8 10 II. 16 20
what is the atomic mass of an unidentified element that has 2 naturally occurring isotopes with the following masses and natural abundances? Isotope 1: 44.8776 amu, 32.88%isotope 2: 46.9443 amu, 67.12%