Define weighted average and average in Chemistry and explain the difference between the two. To find the average atomic mass of neon, we will use the equation above and take the abundance of thefirst isotope times the mass of the first isotope plus the abundance of the second isotope times the massof the second isotope plus the abundance of the third isotope times the mass of the third isotope.However, you might recall from your math courses that when you use a percentage in a calculation youalways want to use the decimal form, meaning you must first divide the percentage by 100. The equationwould then look like:= (0.9048 x 19.9924 amu) + (0.0027 x 20.9938 amu) + (0.0925 x 21.9914 amu)0.0516 amu2.034 amu=18.089 amu= 20.18 amu++ Since the abundances are not equal, we cannot do a typical simple average where we just add them uand divide by two. Instead, we need to perform a weighted average. The formula to calculate theaverage atomic mass is:average atomic mass=(relative abundance x mass of isotope)Remember that is the symbol for sum. In other words, we will take the sum of the relative abundanceof each isotope multiplied by its mass.ExampleNeon has three naturally occurring isotopes.SymbolNe-20Ne-21Ne-22Mass Isotopic mass Percent naturalnumber (amu)20212219.992420.993821.9914abundance90.48%0.27%...

Average is a summation of quantities, divided by the total quantities, to get a single number. For…

Answered: Define weighted average and average in…

Science

Chemistry

Define weighted average and average in Chemistry and explain the difference between the two.

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 43E: The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has...

See similar textbooks

Related questions

Q: The kinetics of the reaction below were studied and it was determined that the reaction rate:…

Q: How many neutrons are in an atom of aluminum (Al) with a mass number of 27?

Q: Draw the organic product of the Bronsted acid-base reaction. Include all lone pairs and charges as…

Q: A CI F K A C E G CH3 HO HJ HH IFC BI H Br D CIG These atoms will interact with methyl in a…

A: the atoms that will sterically interact with the methyl group in a 1,3‑diaxial fashion.

Q: Mass of CuX= 0.2529 g Mass of Cu2+ = 0.0644 g Atomic mass of Cu= 63.55 g/mol a) Calculate the…

A: Number of moles is calculated by dividing the given mass with molecular mass. Mass of CuX= 0.2529 g…

Q: 4 Explain why the boiling point of propanamide, CH3CH₂CONH₂, is considerably higher than the boiling…

A: Given two compounds are propanamide and N,N-dimethylformamide .…

Q: 1. How many grams of NH4OH must be dissolved in enough water to make 350 mL solution such that the…

A: we have to calculate the mass of NH4OH to prepare the solution

Q: 0-04 Mana CI + NaOH O gluma H + NaOH CI + AICI3 glavna This H + AICI 3

A: Appropriate reagent can be found by applying correct reaction mechanism.

Q: Calculate the number of O atoms in 0.0136 g of CaSO4 2H₂O. x 10 O atoms (Enter your answer in…

A: Answer: Given data: Mass of CaSO4.2H2O m=0.0136g

Q: Statement 1: Molecular solids have relatively low melting points. Statement 2: Molecular solids are…

A: We have given two statements about molecular solids.We have to choose which statement is true or…

Q: How many electrons are in an electrically-neutral atom of aluminum (Al) with a mass number of 27?

Q: Ideal Gas Law XT₁ 1.5 atm x 2.99 k R=0.082 nrT 10) Calculate the pressure, in atmospheres, exerted…

Q: The partial pressure of O₂ in your lungs varies from 25 mm Hg to 40 mm Hg. What mass of O₂ can…

A: • Henry's law :- Henry's law tells us the quantity of gas that can be dissolved in a liquid. Higher…

Q: A metal crystallizes in a cubic close-packed structure also known as the face-centered cubic…

Q: What is the solubility of nitrogen (in units of grams per liter) in water at 25 °C, when the N2 gas…

Q: Of the following, which is the most reasonable last step of the synthesis to make the desired target…

Q: An analytical chemist weighs out 0.252 g of an unknown diprotic acid into a 250 ml. volumetric flask…

A: Given -> Weight of 0.252 gm Volume of diprotic acid = 250 ml Molarity of NaOH = 0.0500 M…

Q: The specific heat capacity of silver is 0.235 J/g. K. Its melting point is 962 °C, and its enthalpy…

Q: The 1H NMR spectrum shown represents which compound? 5 1 Н | H-C н H 4 a) 2 Н | - С - ОН Н 3 PPM нн…

Q: Part 2: Rotation Barriers: Rank the rotational barriers relative to the highlighted bonds, with 1…

A: As , known more bulkier is the group more is the barrier provided for its rotation around bond.

Q: What is the molecular geometry about the central atom in the angle shown in the molecule below? H H…

Q: 350 k 2) A gas occupies 1.00 L at 0.00°C. What is the volume at 333.0 °C? V₂ = V₁ Ta V₁=1.00L

A: Answer-2 According to Charles law on keeping the pressure of a system constant, volume of gas…

Q: 8. 12 P OPER NEN 20 icomms svig of GOD negen 57-71 noggen 89-10 ZORDRIN t) Assume Dr. Bork gives you…

A: Given in following question in question 8 molecule of sucrose calculate how many grams of sucrose.…

Q: 4-ter-butyl-2methyl heptane draw the stucture

A: Here, we have to draw the structure of 4-tert-butyl-2methyl heptane. NOTE: In the question, it…

Q: Compounds with two carbonyl groups are named as alkane diones, for example: R 2,3-butanedione The…

A: We have given three organic compounds and we are asked to name these organic compounds.Organic…

Q: Using the bond energies provided, calculate the enthalpy (kJ/mol) of the following reaction: C2H4 +…

Q: Problem 2.22 The C-H bond in acetone, (CH3)2C=O, has a pK, of 19.2. Draw two resonance structures…

A: 2.22: The C-H bond in acetone, (CH3)2C=O, has a pKa of 19.2. We need to draw the resonance…

Q: Boc N TS SmIa THF-78°C Boc What is the mechanism of this reaction? It states that it undergoes a…

A: SmI2 reduces alpha-tosyl carbonyl compounds through free radical mechanism.

Q: 2. Given the electrochemical reaction shown, if the standard reduction potential of Ag+ → Ag is…

Q: Predict the major product of the following reaction: (a) RCO,H?

Q: H₂C Name the following compounds propery. HO H.C Acetaphenone b) НО. 0 №=₂0 0 3 Bromo, •thul Ciclo…

A: In IUPAC nomenclature longest carbon chain is arranged at first. Then lowest locant rule is followed…

Q: 11) Calculate the volume, in liters, occupied by each of the following: a. 2.00 moles of H₂ at 300.…

A: We will solve this problem using ideal gas equation

Q: 3. Draw a reaction coordinate diagram for ... an exergonic reaction Free energy Progress of the…

A: We can draw reaction coordinate diagrams by considering reactants and products free energies.

Q: what ie the position of the group 1 and 2 shown?

Q: Which of the following terms or phrases describe the OIL DROP experiment? charged plates discovered…

Q: 4. Calculate the standard potential energy for this cell: 2Na(s) + Fe²(aq) ---> 2Na²+ (aq) + Fe(s)

Q: metallic solid crystallizes in a body-centered cubic arrangement. Calculate the radius of its atom…

Q: Calculate the solubility of Nickel Hydroxide, Ni(OH), in g/L 25C. Assume a large excess of the…

A: The solubility expression for Ni(OH)2 is Ni(OH)2 (s) <-------> Ni+2 (aq) + 2 OH– (aq) At…

Q: A solution prepared by dissolving 6.95×10−3g6.95×10−3g of protein in enough water to give 0.0300 L…

Q: What is the difference between the molecules of soaps and detergents, chemically? Explain the…

A: The difference between the molecules of soaps and detergents, chemically is given below

Q: Propose an efficient synthesis the following transformation: The transformation above can be…

Q: STARTING AMOUNT X Percocet contains oxycodone at varying strengths. Every strength also contains 325…

A: Given data is The strength of Oxycodone tablet is 325 mg Maximum daily dose of Oxycodone = 3.9 g…

Q: Which of the following terms or phrases describe the CATHODE RAY TUBE experiment? discovered the…

A: Cathode ray tube experiment was performed by Thomson. He discovered electron and m/e ratio to the…

Q: Starch is the indicator in 3 component system Select one: True False

A: Starch is a viable indicator in the titration process because it turns deep dark blue when iodine is…

Q: Draw a sketch of metallic bonds and label the metal cations and delocalized electrons. List one…

A: Metallic bonds occur between metallic ions and sea of electrons . Ionic bonds are forces of…

Q: Consider the following equation: KOH(s) + CO₂(g) → K₂CO₃(s) + H₂O(l) Calculate the mass in grams of…

Q: Calculate the partial pressure of PCl5 at 1.00 bar total pressure and 400 K:…

A: The original reaction mixture contains 1.00 mol PCl3 and 2.00 mol Cl2. Let the Gibbs free energy…

Q: Write a balanced equation for the following: 1. Mg | Mg2+ || Set | Sc 2. Sn Sn²+ || Pb²+ | Pb

Q: 11) Calculate the volume, in liters, occupied by each of the following: a. 2.00 moles of H₂ at 300.…

Q: F sp² hybridized trigonal planar Problem 2.30 Which species are Lewis bases? a. NH3 b. CH3CH₂CH3 c.…

A: According to the Lewis definition, the species which donates lone pair of electrons acts as a Lewis…

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

100%

Define weighted average and average in Chemistry and explain the difference between the two.

To find the average atomic mass of neon, we will use the equation above and take the abundance of the
first isotope times the mass of the first isotope plus the abundance of the second isotope times the mass
of the second isotope plus the abundance of the third isotope times the mass of the third isotope.
However, you might recall from your math courses that when you use a percentage in a calculation you
always want to use the decimal form, meaning you must first divide the percentage by 100. The equation
would then look like:
= (0.9048 x 19.9924 amu) + (0.0027 x 20.9938 amu) + (0.0925 x 21.9914 amu)
0.0516 amu
2.034 amu
=
18.089 amu
= 20.18 amu
+
+

Since the abundances are not equal, we cannot do a typical simple average where we just add them u
and divide by two. Instead, we need to perform a weighted average. The formula to calculate the
average atomic mass is:
average atomic mass=(relative abundance x mass of isotope)
Remember that is the symbol for sum. In other words, we will take the sum of the relative abundance
of each isotope multiplied by its mass.
Example
Neon has three naturally occurring isotopes.
Symbol
Ne-20
Ne-21
Ne-22
Mass Isotopic mass Percent natural
number (amu)
20
21
22
19.9924
20.9938
21.9914
abundance
90.48%
0.27%
...

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1 Average

VIEW

Step 2 Weighted Average

VIEW

Step 3 Difference between Average and Weighted Average

VIEW

Step by step

Solved in 3 steps

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

A jar contains some number of jelly beans. To find out precisely how many are in the jar, you could dump them out and count them. How could you estimate their number without counting each one? (Chemists need to do just this kind of bean counting when they work with atoms and molecules. Atoms and molecules are too small to count one by one, so chemists have worked out other methods to determine the number of atoms in a sample.)
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
The mass spectrum of nitrogen dioxide is illustrated here. (a) Identify the cations present for each of the four peaks in the mass spectrum. (b) Does the mass spectrum provide evidence that the two oxygen atoms are attached to a central nitrogen atom (ONO), or that an oxygen atom is at the center (NOO)? Explain.
The following chart shows a general decline in abundance with increasing mass among the first 30 elements. The decline continues beyond zinc. Notice that the scale on the vertical axis is logarithmic, that is, it progresses in powers of 10. The abundance of nitrogen, for example, is 1/10,000 (1/104) of the abundance of hydrogen. All abundances are plotted as the number of atoms per 102 atoms of H. (The fact that the abundances of Li, Be, and B, as well as those of the elements near Fe, do not follow the general decline is a consequence of the way that elements are synthesized in stars.) (a) What is the most abundant main group metal? (b) What is the most abundant nonmetal? (c) What is the most abundant metalloid? (d) Which of the transition elements is most abundant? (e) Which halogens are included on this plot, and which is the most abundant?
Reference Section 5-2 to find the atomic masses of 12C and 13C, the relative abundance of 12C and 13C in natural carbon, and the average mass (in u) of a carbon atom. If you had a sample of natural carbon containing exactly 10,000 atoms, determine the number of 12C and 13C atoms present. What would be the average mass (in u) and the total mass (in u) of the carbon atoms in this 10,000-atom sample? If you had a sample of natural carbon containing 6.0221 1023 atoms, determine the number of 12C and 13C atoms present What would be the average mass (in u) and the total mass (in u) of this 6.0221 1023 atom sample? Given that 1 g = 6.0221 1023 u, what is the total mass of I mole of natural carbon in units of grams?
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 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?
Use the law of conservation of mass to determine which numbered box(es) represent(s) the product mixture after the substances in the unnumbered box undergo a reaction.
A cube of sodium has length 1.25 in. How many atoms are in that cube? (Note: dNa=0.968g/cm3.)
Europium has two stable isotopes, 151Eu and 153Eu, with masses of 150.9197 u and 152.9212 u, respectively. Calculate the percent abundances of these isotopes of europium.