Element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is amu. Isotope Abundance 38X Mass 5.07 37.919 39X 15.35 39.017 42X 79.85 42.111 O 33.33 O 38.64 O 39.07 O 39.68 O 41.54

Element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is amu. Isotope Abundance 38X Mass 5.07 37.919 39X 15.35 39.017 42X 79.85 42.111 O 33.33 O 38.64 O 39.07 O 39.68 O 41.54

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

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 44E: The element silver (Ag) has two naturally occurring isotopes: 109 Ag and 107Ag with a mass of...

See similar textbooks

Related questions

Q: A hydrate is a compound with water molecules incorporated into its crystal structure. In an…

A: The question is based on the concept of analytical chemistry.We need to calculate percentage of…

Q: Naturally occurring chlorine is 75.78% 35Cl (atomic mass 34.969 u) and 24.22% 37Cl (atomic mass…

A: Given : Atomic mass of lighter isotope i.e 35Cl (A1) = 34.969 u Percentage abundance of lighter…

Q: A sample has 8.63 x 10 atoms of boron. How many moles of boron does this represent? O1.41 .014 O…

A: Given : Number of atoms of boron = 8.63 X 1021 atoms

Q: A student, Ken, is given a mixture containing two nitrate compounds. The mixture includes NaNO3 and…

A: Mixture consists of two nitrate compounds NaNO3 and Ca(NO3)2. Mass Percentage of NO3 in the mixture…

Q: Based on the law of conservation of mass, how many grams of hydrogen gas, x, are formed by the…

A: Given, 66.0 g zinc + 72.9 g hydrochloric acid produces 136.3 g zinc chloride+ x g hydrogen gas. We…

Q: Calculate the mass, in kg, of sample. 8.15x10^27 nickel atoms

A: The mass of sample. 8.15x10^27 nickel atoms is to be calculated

Q: Macmillan Learning, On another planet, the isotopes of titanium have the given natural abundances.…

A: Average atomic mass : The average atomic mass of an element is the sum of the atomic masses of it's…

Q: The atomic weight of bromine is 79.904, yet no atom of bromine weighs 79.904 amu. Why is this true?

A: Given : The atomic weight of bromine is 79.904, yet no atom of bromine weighs 79.904 amu.

Q: he average atomic masses of some elements may vary, depending upon the sources of their ores.…

A: Explanation Solution Two substances, the percentage of each isotope, are unidentified. As both…

Q: Iron exists in nature as a mixture of predominantly three isotopes: ⁵⁴₂₆Fe (53.94 amu), ⁵⁶₂₆Fe…

A: We have to calculate the percentage of rarest of three isotopes.

Q: A student has a sample of zinc that weighs 22.19 g. How many zinc atoms are in this amount of zinc?…

A: The Number of atom present in one mole of an element is equal to the Avogadro's number (6.022×1023…

Q: Which sample contains the greatest number of atoms? O 102 g Ag O 189 g Ir O 18 g O O 53 g Fe

A: The number of moles is defined as the ratio of a given mass to molar mass. No. of moles =Given…

Q: Some of the formulas could be either molecular or empirical formulas; however, some can only be…

Q: None

A: To calculate the average atomic mass of titanium on the given planet, you will use the natural…

Q: Assume magnesium has three major isotopes in nature as shown in the table below. Fill in the missing…

Q: Table 1: Molar masses of common rock forming elements Atomic Mass (amu) 28.09 Element Oxide (1)…

A: We can identify the valency of oxide are as follows Suppose the oxide formula is = MaOb(=2) Here,…

Q: What is the mass of 3.30 x 1023 atoms of silver, Ag? 25.8 g 59.1 g 85.7 g 197 g 0.549 g

A: We will use formula of mole and mass to get answer. Number of atom = 3.3×1023

Q: n element consists of 1.40% of an isotope with mass 203.9730 u, 24.10% of an isotope with mass…

A: Given that, Element consists of 1.40% of an isotope with mass 203.9730 u, 24.10% of an isotope with…

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: 9. Complete the columns in the table: formula: Sno2 P203 H3PO4(ag) calcium hydrogen name: chloric…

Q: 22 Calculate the mass of 3.0 × 1044 atoms of sulfur. O 1.6 g O 16 g O 160 g O 0.16 g

Q: There are two gas compounds that are made out of element A and B. This is the mass percentage of…

A: Given: Mass percentage: Compound 1: 30.43% A, 69.57% B Compound 2: 63.64% A, 36.36% B

Q: Imagine that you have discovered several stable isotopes of a new element, which you call element X.…

Q: Calculate the mass, in kg, of sample. 7.55x10^26 cadmium atoms

Q: The average atomic mass of silicon is 28.0855 u. What percentage of silicon atoms are 29Si? Assume…

A: average weight= f1m1+f²m2+f3m3 F= fraction of natural abundance of isotopes by 100 m= mass of…

Q: 7. Which of the following is the molecular formula of a sample of a compound containing 30.46%…

A: Please find your solution below : Molecular formula of any compound is an expression about the…

Q: How many helium (He) atoms are there in 3.75 moles of helium? 3.75 x 1023 atoms 3.99 x 1025 atoms…

A: You have given - Moles of He = 3.75 mol

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

Q: Bromine and chlorine react to form simple diatomic molecules in a 1:1 ratio, BrCl. The natural…

A: The least common form of BrCl is the molecule that is made from each of the Br and Cl atoms…

Q: Calculate the mass, in grams, of sample. 2.82x10^22 helium atoms

Q: A certain compound X is composed of 70.53% carbon, 13.02% hydrogen, and the remainder is nitrogen.…

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

A: 1.Average atomic mass is the weighted average mass of the sample that occure in nature. 2. Here the…

Q: A 2.58 g sample of a compound consisting of carbon, hydrogen, oxygen, nitrogen, and sulfur was…

Q: A student, Ken, is given a mixture containing two sulfate compounds. The mixture includes K2SO4 and…

A: Given mixture is K2SO4 and BaSO4. The mixture is 52.12 % SO4 by mass. Molar mass of…

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…

Concept explainers

Atoms and Molecules

An atom is the smallest unit of an element that possesses all the properties of that particular element. Molecules are the smallest unit of a substance that possess all the properties of that particular substance.

Question

Element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table below. The average atomic mass of the element is
amu
Isotope Abundance
Mass
38X
5.07
37.919
39X
15.35
39.017
42X
79.85
42.111
O 33.33
O 38.64
O 39.07
O 39.68
O 41.54

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.
An element X bas five major isotopes, which are listed below along with their abundances. What is the element? Isotope Percent Natural Abundance Mass (u) 46x 8.00% 45.95232 47x 7.30% 46.951764 48x 73.80% 47.947947 49x 5.50% 48.947841 50x 5.40% 49.944792
Argon has three naturally occurring isotopes: 0.3336% 36Ar, 0.063% 38Ar, and 99.60% 40Ar. Estimate the average atomic mass of argon. If the masses of the isotopes are 35.968 u, 37.963 u, and 39.962 u, respectively, calculate the average atomic mass of natural argon.
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.
The element rhenium (Re) bas two naturally occurring isotopes, 185Re and 187Re, with an average atomic mass of 186.207 u. Rhenium is 62.60% 187Re, and the atomic mass of 187Re is 186.956 u. Calculate the mass of 185Re.
When a sample of phosphorus burns in air, the compound P4O10 forms. One experiment showed that 0.744 g of phosphorus formed 1.704 g of P4O10. Use this information to determine the ratio of the atomic weights of phosphorus and oxygen (mass P/mass O). If the atomic weight of oxygen is assumed to be 16.000, calculate the atomic weight of phosphorus.
The atomic masses in die periodic table are relative masses and average masses. Explain.
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.
Early tables of atomic weights (masses) were generated by measuring the mass of a substance that reacts with 1.00 g of oxygen. Given the following data and taking the atomic mass of hydrogen as 1.00, generate a table of relative atomic masses for oxygen, sodium, and magnesium. Element Mass That Combines with 1.00Oxygen Assumed Formula Hydrogen 0.126g HO Sodium 2.875g Nao Magnesium 1.500g Mgo
Early tables of atomic weights (masses) were generated by measuring the mass of a substance that reacts with 1.00 g of oxygen. Given the following data and taking the atomic mass of hydrogen as 1.00, generate a table of relative atomic masses for oxygen, sodium, and magnesium. Element Mass That Combines with 1.00g Oxygen Assumed Formula Hydrogen 0.126 g HO Sodium 2.875 g NaO Magnesium 1.500 g MgO How do your values compare with those in the periodic table? How do you account for any differences?
What is the mass of one 16O atom, in grams? (The mass of an 16O atom is 15.995 u.)
Neon has three stable isotopes, one with a small abundance. What are the abundances of the other two isotopes? 20Ne, mass = 19.992435 u; percent abundance = ? 21Ne mass = 20.993843 u; percent abundance = 027% 22Ne mass = 21.991383 u: percent abundance = ?