HCF of three numbers

Average Atomic Mass Calculator

Chemistry Engineering Financial Health More >>

↳

Basic Chemistry Analytical chemistry Atmospheric Chemistry Atomic structure More >>

⤿

Determination of Equivalent Mass Important Formulas of Basic Chemistry

✖Ratio Term of Isotope A represents the quantity that denotes the ratio relation Isotope A has to Isotope B.ⓘ Ratio Term of Isotope A [m]			+10% -10%
✖Atomic Mass of Isotope A is the quantity of matter contained in an atom of the isotope A.ⓘ Atomic Mass of Isotope A [a]			+10% -10%
✖Ratio Term of Isotope B represents the quantity that denotes the ratio relation Isotope B has to Isotope A.ⓘ Ratio Term of Isotope B [n]			+10% -10%
✖Atomic Mass of Isotope B is the quantity of matter contained in an atom of the isotope B.ⓘ Atomic Mass of Isotope B [b]			+10% -10%

✖Average Atomic Mass is defined as the average of the atomic masses of two isotopic compositions of the same element.ⓘ Average Atomic Mass [A.M_avg]

⎘ Copy

👎

Formula

LaTeX

Reset

👍

Download Basic Chemistry Formula PDF PDF Image

Average Atomic Mass Solution

STEP 0: Pre-Calculation Summary

Formula Used

Average Atomic Mass = (Ratio Term of Isotope A*Atomic Mass of Isotope A+Ratio Term of Isotope B*Atomic Mass of Isotope B)/(Ratio Term of Isotope A+Ratio Term of Isotope B)
A.M_avg = (m*a+n*b)/(m+n)
This formula uses 5 Variables

Variables Used

Average Atomic Mass - (Measured in Kilogram) - Average Atomic Mass is defined as the average of the atomic masses of two isotopic compositions of the same element.
Ratio Term of Isotope A - Ratio Term of Isotope A represents the quantity that denotes the ratio relation Isotope A has to Isotope B.
Atomic Mass of Isotope A - (Measured in Kilogram) - Atomic Mass of Isotope A is the quantity of matter contained in an atom of the isotope A.
Ratio Term of Isotope B - Ratio Term of Isotope B represents the quantity that denotes the ratio relation Isotope B has to Isotope A.
Atomic Mass of Isotope B - (Measured in Kilogram) - Atomic Mass of Isotope B is the quantity of matter contained in an atom of the isotope B.

STEP 1: Convert Input(s) to Base Unit

Ratio Term of Isotope A: 3 --> No Conversion Required
Atomic Mass of Isotope A: 34.9688 Gram --> 0.0349688 Kilogram (Check conversion here)
Ratio Term of Isotope B: 0.99 --> No Conversion Required
Atomic Mass of Isotope B: 36.965 Gram --> 0.036965 Kilogram (Check conversion here)

STEP 2: Evaluate Formula

Substituting Input Values in Formula

A.M_avg = (m*a+n*b)/(m+n) --> (3*0.0349688+0.99*0.036965)/(3+0.99)

Evaluating ... ...

A.M_avg = 0.0354640977443609

STEP 3: Convert Result to Output's Unit

0.0354640977443609 Kilogram -->35.4640977443609 Gram (Check conversion here)

FINAL ANSWER

35.4640977443609 ≈ 35.4641 Gram <-- Average Atomic Mass

(Calculation completed in 00.004 seconds)

You are here -

Home » Chemistry » Basic Chemistry » Average Atomic Mass

Credits

Created by SUDIPTA SAHA

ACHARYA PRAFULLA CHANDRA COLLEGE (APC), KOLKATA

SUDIPTA SAHA has created this Calculator and 100+ more calculators!

Verified by Soupayan banerjee

National University of Judicial Science (NUJS), Kolkata

Soupayan banerjee has verified this Calculator and 900+ more calculators!

< Basic Chemistry Calculators

Change in Boiling Point of Solvent

LaTeX Go Change in Boiling Point of Solvent = Molal Boiling Point Elevation Constant*Molal Concentration of Solute

Bond Order

LaTeX Go Bond Order = (1/2)*(Number of Bonding Electrons-Number of Antibonding Electrons)

Boiling Point

LaTeX Go Boiling Point = Boiling Point of Solvent*Change in Boiling Point of Solvent

Percent by Weight

LaTeX Go Percent By Weight = Gram of Solute/100 g of Solution

Average Atomic Mass Formula

LaTeX Go

Average Atomic Mass = (Ratio Term of Isotope A*Atomic Mass of Isotope A+Ratio Term of Isotope B*Atomic Mass of Isotope B)/(Ratio Term of Isotope A+Ratio Term of Isotope B)
A.M_avg = (m*a+n*b)/(m+n)

What is Atomic Mass?

The mass of an atom of a chemical element expressed in atomic mass units. It is approximately equivalent to the number of protons and neutrons in the atom or to the average number allowing for the relative abundances of different isotopes.

What is Average Atomic Mass?

The average atomic mass of an element is the sum of the masses of its isotopes, each multiplied by its natural abundance (the decimal associated with percent of atoms of that element that are of a given isotope).
The average atomic mass of an element can be found on the periodic table, typically under the elemental symbol. When data are available regarding the natural abundance of various isotopes of an element, it is simple to calculate the average atomic mass.
For helium, there is approximately one isotope of Helium-3 for every million isotopes of Helium-4; therefore, the average atomic mass is very close to 4 amu (4.002602 amu).Chlorine on the other hand, consists of two major isotopes, one with 18 neutrons (75.77 percent of natural chlorine atoms) and one with 20 neutrons (24.23 percent of natural chlorine atoms). The atomic number of chlorine is 17 (it has 17 protons in its nucleus).

How to Calculate Average Atomic Mass?

Average Atomic Mass calculator uses Average Atomic Mass = (Ratio Term of Isotope A*Atomic Mass of Isotope A+Ratio Term of Isotope B*Atomic Mass of Isotope B)/(Ratio Term of Isotope A+Ratio Term of Isotope B) to calculate the Average Atomic Mass, The Average Atomic Mass formula is defined as average of the atomic masses of element which exists in two different isotopic forms, namely 'a' and 'b' present in the ratio m:n. Average Atomic Mass is denoted by A.M_avg symbol.

How to calculate Average Atomic Mass using this online calculator? To use this online calculator for Average Atomic Mass, enter Ratio Term of Isotope A (m), Atomic Mass of Isotope A (a), Ratio Term of Isotope B (n) & Atomic Mass of Isotope B (b) and hit the calculate button. Here is how the Average Atomic Mass calculation can be explained with given input values -> 35464.1 = (3*0.0349688+0.99*0.036965)/(3+0.99).

FAQ

What is Average Atomic Mass?

The Average Atomic Mass formula is defined as average of the atomic masses of element which exists in two different isotopic forms, namely 'a' and 'b' present in the ratio m:n and is represented as A.M_avg = (m*a+n*b)/(m+n) or Average Atomic Mass = (Ratio Term of Isotope A*Atomic Mass of Isotope A+Ratio Term of Isotope B*Atomic Mass of Isotope B)/(Ratio Term of Isotope A+Ratio Term of Isotope B). Ratio Term of Isotope A represents the quantity that denotes the ratio relation Isotope A has to Isotope B, Atomic Mass of Isotope A is the quantity of matter contained in an atom of the isotope A, Ratio Term of Isotope B represents the quantity that denotes the ratio relation Isotope B has to Isotope A & Atomic Mass of Isotope B is the quantity of matter contained in an atom of the isotope B.

How to calculate Average Atomic Mass?

The Average Atomic Mass formula is defined as average of the atomic masses of element which exists in two different isotopic forms, namely 'a' and 'b' present in the ratio m:n is calculated using Average Atomic Mass = (Ratio Term of Isotope A*Atomic Mass of Isotope A+Ratio Term of Isotope B*Atomic Mass of Isotope B)/(Ratio Term of Isotope A+Ratio Term of Isotope B). To calculate Average Atomic Mass, you need Ratio Term of Isotope A (m), Atomic Mass of Isotope A (a), Ratio Term of Isotope B (n) & Atomic Mass of Isotope B (b). With our tool, you need to enter the respective value for Ratio Term of Isotope A, Atomic Mass of Isotope A, Ratio Term of Isotope B & Atomic Mass of Isotope B and hit the calculate button. You can also select the units (if any) for Input(s) and the Output as well.

Home

FREE PDFs

🔍 Search