A certain element X has four isotopes. • 4.350% of X has a mass of 49.94605 amu. • 83.79% of X has a mass of 51.94051 amu. • 9.500% of X has a mass of 52.94065 amu. 2.360% of X has a mass of 53.93888 amu. What is the average atomic mass of element X? Express your answer numerically to four significant figures. ► View Available Hint(s) 52.00 amu Submit Previous Answers Correct Part C What is the identity of element X from Part B? Express your answer as a chemical symbol.

A certain element X has four isotopes. • 4.350% of X has a mass of 49.94605 amu. • 83.79% of X has a mass of 51.94051 amu. • 9.500% of X has a mass of 52.94065 amu. 2.360% of X has a mass of 53.93888 amu. What is the average atomic mass of element X? Express your answer numerically to four significant figures. ► View Available Hint(s) 52.00 amu Submit Previous Answers Correct Part C What is the identity of element X from Part B? Express your answer as a chemical symbol.

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

a) On earth, tin has 10 different stable isotopes. The heaviest, 124Sn makes up 5.80% of naturally occurring tin atoms. How many atoms of 124Sn are present in 38.3g of a natural sample of tin? b) Considering 124Sn has an isotopic mass of 123.905 amu, calculate the mass of this isotope in the sample.
12) The smallest sample of carbon atoms that can be observed with the naked eye has a mass of approximately 2 × 10-8 g. Given that 1 g = 6.02 × 1023 amu, and that carbon has an atomic weight of 12.01 amu, determine the number of carbon atoms present in the sample. a) 1 × 1017 b) 6 × 1023 c) 1 × 1016 d) 1 × 1015
An unknown element is determined to have two naturally occurring isotopes. Isotope 1 is 68.11% abundant and has a mass of 68.925580 amu, and isotope 2 has a mass of 70.9247005 amu. Determine the atomic mass of the unknown element. Express your answer to four significant figures.
Element A has two isotopes. The first isotope is present 19.41% of the time and has a mass of 231.12. The second isotope has a mass of 193.24. Calculate the atomic mass of element A.
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.
A new synthetic element is found to have two isotopes. One isotope has an abundance of 68.2% and a mass of 296.5 amu. The other isotope has a mass of 299.6 amu. What atomic mass should be written on the periodic table for this new element?
Copper has two naturally occurring isotopes: 69.17% of Cu-63 (mass 62.93 amu) and 30.83% of Cu-65 (mass 64.93 amu). Calculate the average atomic mass of copper.
Hi! I am on the study section that my teacher has provided to help us prepare for our test tomorrow if we choose to use it! I am having a hard time with this question and would like to get a better understanding before the test tomorrow.
Potassium has 2 naturally occurring isotopes. 39K has a mass of 38.96 amu and accounts for 93.26% of potassium atoms. What is the mass of an atom of the second potassium isotope?
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?