The element X has isotopes. The masses (atomic mass unit) and % abundances of the isotopes are given in the table below. The average atomic mass of the :element in atomic mass unit is table Mass Abundance Isotope 220.9 74.22 221x 220.0 12.78 220x 218.1 13.00 218X 219.7 220.4 218.5 221.4

The element X has isotopes. The masses (atomic mass unit) and % abundances of the isotopes are given in the table below. The average atomic mass of the :element in atomic mass unit is table Mass Abundance Isotope 220.9 74.22 221x 220.0 12.78 220x 218.1 13.00 218X 219.7 220.4 218.5 221.4

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 42E: The element silver (Ag) has two naturally occurring isotopes: 109 Ag and 107Ag with a mass of...

See similar textbooks

Related questions

Q: Relative number of atoms The stable isotopes of iron are 54F., 56FE, 57Fe, and 58F.. The mass…

Q: Element X reacts with chlorine to form a compound with the formula of X2Cl3. This compound contains…

A: Relative atomic mass: Cl = 35.5 g/mol

Q: The element X has three naturally occurring isotopes. The isotopic masses (amu) and % abundances of…

Q: The atomic masses of 6 Li and 7 Li are 6.0151 amu and 7.0160 amu, respectively. Calculate the…

A: The isotopes of Lithium are Li6 and Li7 whose atomic masses are 6.0151 amu and 7.0160 amu…

Q: Lithium forms compounds which are used in dry cells and storage batteries and in high-temperature…

A: The variants of any element containing dissimilar neutrons number but similar protons number (atomic…

Q: Silicon, which makes up about 25% of Earth's crust by mass, is used widely in the modern electronics…

A: Average atomic mass- Naturally occurring element exists as mixture isotopes. Isotopes are with…

Q: An element X exists as two isotopes - 46X and 49X and weigh 45.95 amu and 48.95 amu, respectively.…

A: Given :- Atomic wt.of 46X = 45.95 amu Atomic wt.of 49X = 48.95 amu Average atomic wt.of X = 46.66…

Q: Element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes…

Q: Gallium has two naturally occurring isotopes, 69Ga (isotopic mass = 68.9256 amu, abundance = 60.11%)…

A: Isotopes are atoms of same elements which have same atomic number but different mass number. There…

Q: What is the mass percentage of phosphorus in a sample of 8.53 phosphorus oxychloride containing a…

A: Mass percentage of phosphorus = 20.16 %

Q: Potassium has three stable isotopes, potassium-39, potassium-40, and potassium-41. calculate the…

A: Potassium exhibit three stable isotopes, Potassium- 39, potassium - 40 and potassium - 41. Here, we…

Q: Bronze is an alloy with the following composition: Component Copper Nickel Zinc mass percentage 52.0…

A: Given Mass percentage of Cu = 52% Total mass of sample = 2 gram mass of copper =…

Q: The two isotopes of potassium with significant abundance in nature are ³⁹K (isotopic mass 38.9637…

A: NOTE : The sum of abundance of the two isotopes should be 100 %. And since the abundance values do…

Q: The atomic masses of 6Li and 7Li are 6.0151 amu and 7.0160 amu, respectively. Calculate the natural…

A: Given data contains, Atomic mass of 6Li is 6.0151 amu. Atomic mass of 7Li is 7.0160 amu. Average…

Q: The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the…

Q: 8- Bromine (Br) has two isotopes, with masses of 78.92 and 80.92 amu. The natural abundance of the…

Q: An element X has the following masses and % abundance. 35X (34.97 amu 75.8%) and 37X ( 36.99amu…

A: Answer :- amu (atomic mass unit) - It is the unit to express the atomic mass. % abundance - It is…

Q: Iron has three major isotopes: 54Fe (atomic mass = 53.9396 u; abundance 5.85%), 56Fe (atomic mass =…

A: Isotopes are atoms of same elements which have same atomic number but different mass number.…

Q: Page |99 SUBATOMIC PARTICLES AND ISOTOPES Complete Symbol Atomic Mass Number of Number of Number of…

Q: The element X has two naturally occurring isotopes. The masses (amu) and % abundances of the…

Q: A 6.55 g sample of calcium sulfide was decomposed into its constituent elements, producing 3.64 g of…

A: According to the law of constant composition, for any particular chemical compound, all samples of…

Q: A 12.49 g sample of NaBr contains 22.34% Na by mass. Considering the law of constant composition…

A: Average atomic mass of the element = Mass of one isotope of the element x % natural abundance + Mass…

Q: The natural abundance for element "X's" isotopes are: 19.9% 10X (10.013 amu) and 80.1% 11X…

A: Given, an element X and has two natural isotopes with abundance of19.9% of X10(10.013 amu) and 80.1%…

Q: On another planet, the isotopes of titanium have the given natural abundances. Abundance Mass (u)…

Q: Unknown element, Element X, exists in nature as two isotopes: ^{351}351 X has a mass of 350.9196 u…

A: Average atomic mass=∑i=1n (mass of ith isotope)(%abundance of ith isotope)100 where 'i'…

Q: An unknown element is a mixture of isotopes ¹²⁰X and ¹²²X. The average atomic mass of X is 121.47…

A: For an element that exists as a number of isotopes, its atomic mass is calculated by taking an…

Q: Naturally occurring thallium consists of two stable isotopes, Tl-203 and TI-205 atomic masses =…

Q: On another planet, the isotopes of titanium have the given natural abundances. Abundance Mass (u)…

A: Average atomic mass =( m1a1 + m2a2 + m3a3)/100 m = mass of isotopes a= abundance

Q: . Explain the role of relative weight in determining the atomic mass of an element. 2.…

A: 1. The relative weight term is used to the calculate the atomic weight of an element as the weight…

Q: 8- Bromine (Br) has two isotopes, with masses of 78.92 and 80.92 amu. The natural abundance of the…

A: bromine has two isotopes which are Br-79 and Br-81. Given, the mass of Br-79 isotope = 78.92 amu the…

Q: Naturally occurring chlorine is composed of two isotopes: 75.76% Cl-35 (mass 34.9688 amu) and 24.24%…

A: The elements having same atomic number, but different mass number are termed as isotopes. A molecule…

Q: Mg (24.305 amu) consists of three isotopes with the masses 23.9850 amu ,24.9858 amu, and 25.9826.The…

A: We have to predict the percentage abundance of first isotope.

Q: Consider the table below. What is the relative abundance of isotope A? Isotope Abundance A 65 B 115…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: Antimony, Sb (atomic mass 121.760 amu) has two stable isotopes: 121Sb (atomic mass 120.904 amu) and…

Q: On another planet, the isotopes of titanium have the given natural abundances. Abundance Mass (u)…

A: Given : Isotope Abundance Mass (u) 46Ti 78.900 % 45.95263 48Ti 13.800 % 47.94795 50Ti…

Q: Element X has two naturally occurring isotopes, 65X(isotopic mass 64.7471 amu, abundance 28.49%)…

A: Given : Element X has 2 naturally isotopes. Mass of isotope 65X = 64.7471 amu Abundance of 65X =…

Q: Sycamorium Sy, a hypothetical element occurs in three isotopes, who masses and abundances are given…

A: Given: Isotope Mass Abundance Isotope1 297.021 21.9% Isotope2 299.010 33.3% Isotope3…

Q: What is the mass of one atom of I? O 2.107 x 10 22 8. O 3.443 x 1023 O 4.745 x 10-22 g O 6.641x…

A: To find mass for one atom of an element, divide the atomic mass of an element by avogadro number. It…

Q: What is the atomic weight of an element that consists of TWO isotopes as follows: Isotope 1: mass =…

A: Here we have to determine the atomic weights of element is have two isotopes in following abundances…

Q: 8- Bromine (Br) has two isotopes, with masses of 78.92 and 80.92 amu. The natural abundance of the…

Q: The relative abundance and atomic masses are 0.337% (mass = 35.978 amu) 0.063% (mass = 37.963 amu)…

A: Average atomic mass of an element is the sum of the masses of its isotopes each multiplied by its…

Q: The stable isotopes of iron are $4Fe, Fe, $7Fe, and 5"Fe. The mass spectrum of iron looks like the…

A: The given mass spectra of iron is, The relative number of isotope atoms of 54Fe is 5.85. The…

Q: An element has three isotopes. Giving the abundances and relative masses calculate the average…

A: Average atomic mass of an element can be calculated from their relative abundances from the…

Q: The average mass of a boron atom is 10.81. You perform an experiment using mass spectrometry and…

A: Two questions each in nuclear chemistry and inorganic chemistry which are to be answered.

Q: Determine Average Atomic Mass for oxygen: Isotope percentage Abundance Actual Mass O-16 99.762%…

A: Average atomic mass of an element is the sum of masses of its isotopes, each multiplied by its…

Q: In nature, Titanium has five stable isotopes. If the atomic masses and the relative abundances for…

A: Given, the atomic masse and their relative abundance of first four isotopes of Titanium are as…

Q: Silicon is widely used in the semiconductor industry. Its isotopes and abundance are: Si-28 (27.977…

Q: On another planet, the isotopes of titanium have the given natural abundances. Mass (u) Isotope 46…

A: Average atomic mass = m1f1 + m2f2 + m3f3

Q: The element silver (Ag) has two naturally occurring isotopes:109 Ag and 107Ag with a mass of 106.905…

Q: The stable isotopes of iron arc 54Fe, 56Fe, 57Fe, and 58Fe. The mass spectrum of iron looks like the…

A: The mass spectrum of the iron is given as,

Concept explainers

Mass Spectrometry

This process is an instrumental method in which a sample is changed to fast moving positive ions by electron bombardment. The charged particles vary due to their different mass to charge ratio and are estimated with the help of this difference. It is also called mass spectroscopy.

Question

The element X has isotopes. The
masses (atomic mass unit) and %
abundances of the isotopes are
given in the table below. The
average atomic mass of the
:element in atomic mass unit is
table
Mass
Abundance Isotope
220.9
74.22
221x
220.0
12.78
220x
218.1
13.00
218X
219.7
220.4
218.5
221.4

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has a mass of 152.9209 u. The average atomic mass of europium is 151.96 u. Calculate the relative abundance of the two europium isotopes.
The average atomic masses of some elements may vary, depending upon the sources of their ores. Naturally occurring boron consists of two isotopes with accurately known masses ( 10B, 10.0129 amu and 11B, 11.0931 amu). The actual atomic mass of boron can vary from 10.807 to 10.8 19, depending on whether the mineral source is from Turkey or the United States. Calculate the percent abundances leading to the two values of the average atomic masses of boron from these two countries.
A gaseous binary compound has a vapor density that is 2.53 times that of nitrogen at 100°C and atmospheric pressure. When 8.21 g of the gas reacts with AlCl3 at 100°C, 1.62 g gaseous nitrogen is produced, removing all of the nitrogen originally present. (a) Estimate the molecular mass of the gaseous compound. (b) How many nitrogen atoms are there in a molecule of the compound? (c) What is the maximum possible value of the atomic mass of the second element? (d) Are other values possible for the atomic mass of the second element? Use a table of atomic masses to identify the element that best fits the data. (e) What is the molecular formula of the compound?
A gaseous binary compound has a vapor density that is 1.94 times that of oxygen at the same temperature and pressure. When 1.39 g of the gas is burned in an excess of oxygen, 1.21 g water is formed, removing all the hydrogen originally present. (a) Estimate the molecular mass of the gaseous compound. (b) How many hydrogen atoms are there in a molecule of the compound? (c) What is the maximum possible value of the atomic mass of the second element in the compound? (d) Are other values possible for the atomic mass of the second element? Use a table of atomic masses to identify the element that best fits the data. (e) What is the molecular formula of the compound?
The element silver (Ag) has two naturally occurring isotopes: 109 Ag and 107Ag with a mass of 106.905 u. Silver consists of 51.82% 107Ag and has an average atomic mass of 107.868 u. Calculate the mass of 109Ag.
An element consists of 1.40% of an isotope with mass 203.973 u, 24.10% of an isotope with mass 205.9745 u, 22.10% of an isotope with mass 206.9759 u, and 52.40% of an isotope with mass 207.Y766 u. Calculate the average atomic mass, and identify the element.
Both atomic elements and molecular elements exist. Are there such entities as atomic compounds and molecular compounds? If so, provide an example and microscopic drawing. If not, explain why not.
When we refer to doughnuts or cookies, we often refer to 1doz of them, which corresponds to 12. Why is the dozen an inconvenient number when referring to atoms? Why is Avogadros number, 6.0221023, more convenient?
These questions concern the work of J. J. Thomson: From Thomson’s work, which particles do you think he would feel are most important in the formation of compounds (chemical changes) and why? Of the remaining two subatomic particles, which do you place second in importance for forming compounds and why? Come up with three models that explain Thomson’s findings and evaluate them. To be complete you should include Thomson’s findings.
Calculate the nominal mass of each ion. Unless otherwise indicated, use the mass of the most abundant isotope of each element. (a) (b) (c)