Potassium (K) has two stable isotopes: 39 and 41K. Based on the average atomic mass of potassium from the periodic table (39.098 amu). which isotope of potassium would you predict to be more abundant? O potassium-39 is much more abundant O potassium-41 is much more abundant O the two isotopes are roughly equally abundant O the answer cannot be determined from the given information

Potassium (K) has two stable isotopes: 39 and 41K. Based on the average atomic mass of potassium from the periodic table (39.098 amu). which isotope of potassium would you predict to be more abundant? O potassium-39 is much more abundant O potassium-41 is much more abundant O the two isotopes are roughly equally abundant O the answer cannot be determined from the given information

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

please make sure to choose the corerect answer 100%
There are only two naturally-occuring stable isotopes of chlorine, the masses of which are listed in the table below. Use whatever data you need from the ALEKS Periodic Table to calculate the natural abundance of each isotope and complete the table. 35 Round your entry for C1 to 4 significant digits and your entry for isotope 35 Cl 37 Cl mass (amu) 34.969 36.966 natural abundance 1% % ☐x10 X 37 C1 to 4 significant digits. Ś
There are four isotopes of strontium. They have mass number of 84, 86,87 and 33. The atomic mass of strontium is 87.62 amu. What does it say about the relative abundance of isotopes?
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.
12:50 ← d2fcc1b0-17ba-42ff-a... 15/24 SCIENCE (086) 9 જે SCIENCE 224 Science Project Create a comprehensive and informative project on ' Natural resources' in the form of an artistically crafted, decorated project file Include pictures, illustrations,examples, surveys, advertisements, newspaper cuttings and headings etc in your project to make your project appealing, relevant, easy to understand and memorable Keypoints . Introduction to Natural Resources • Air pollution and its causes Water pollution and its causes Soil pollution and its causes . Biogeochemical Cycles 1. Oxygen Cycle 2. Carbon Cycle 3. Nitrogen Cycle 4. Water Cycle Rain and effect of acid rain . Green-house Effect Ozone Layer and reason for ozone depletion Assignment Sheet 1.Look at Fig. 1.1 and suggest in which of the vessels A,B, C or D the rate of evaporation will be the highest? Explain. PDF to Long Images PDF to Images =
The average atomic mass of copper is 63.546 amu. It is composed of copper-63 and copper-65 isotopes. The natural abundance of copper-63 (62.9296 amu) is 69.17%. Show how the natural abundance of copper-65 (64.9278 amu) can be determined two different ways from the given information.
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
An unknown element has two naturally occurring isotopes. Isotope 1 has a mass of 121.0 amu and an abundance of 55.10%. Isotope 2 has a mass of 123.0 amu. What is the atomic mass of the element?
Silver is composed of two isotopes. One isotope has a mass of 106.91 amu and a relative abudance of 51.84%. What is the mass of the other isotope if its relative abundance is 48.16%? Use the average atomic mass of silver in your calculation.