Average Atomic Mass Calculator

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✖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]

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Formula

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Average Atomic Mass

Formula

`"A.M"_{"avg"} = ("m"*"a"+"n"*"b")/("m"+"n")`

Example

`"35.4641g"=("3"*"34.9688g"+"0.99"*"36.965g")/("3"+"0.99")`

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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)

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< 25 Basic Chemistry Calculators

Average Atomic Mass

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)

Determination of Eqv. Mass of Metal using Chloride Formation Method given vol. of Cl at STP

Go Equivalent Mass of Metal = (Mass of Metal/Vol. of Chlorine reacted)*Vol. of Chlorine reacts with eqv. mass of metal

Determination of Equivalent Mass of Metal added using Metal Displacement Method

Go Equivalent Mass of Metal added = (Mass of Metal added/Mass of Metal displaced)*Equivalent Mass of Metal displaced

Determination of Eqv. Mass of Metal using H2 Displacement Method given vol. of H2 displaced at STP

Go Equivalent Mass of Metal = (Mass of Metal/Vol. of hydrogen displaced at STP)*Vol. of Hydrogen displaced at NTP

Determination of Equivalent Mass of Base using Neutralisation Method

Go Equivalent mass of bases = Weight of bases/(Vol. of acid required for neutralisation*Normality of acid used)

Determination of Equivalent Mass of Acid using Neutralization Method

Go Equivalent mass of acids = Weight of acid/(Vol. of base required for neutralisation*Normality of base used)

Determination of Equivalent Mass of Metal using Oxide formation Method given vol. of Oxygen at STP

Go Equivalent Mass of Metal = (Mass of Metal/Vol. of Oxygen displaced)*Vol. of oxygen combined at STP

Mole Fraction

Go Mole Fraction = (Number of Moles of Solute)/(Number of Moles of Solute+Number of Moles of Solvent)

Equivalent Mass of Metal using Hydrogen Displacement Method

Go Equivalent Mass of Metal = (Mass of Metal/Mass of Hydrogen Displaced)*Equivalent Mass of Hydrogen

Sensible Heat

Go Sensible Heat = 1.10*Rate of Flow of Air Entering Inside*(Outside Temperature-Inside Temperature)

Determination of Equivalent Mass of Metal using Chloride Formation Method

Go Equivalent Mass of Metal = (Mass of Metal/Mass of Chlorine reacted)*Equivalent Mass of Chlorine

Determination of Equivalent Mass of Metal using Oxide formation Method

Go Equivalent Mass of Metal = (Mass of Metal/Mass of Oxygen displaced)*Equivalent Mass of Oxygen

Partition Coefficient

Go Partition Coefficient = Concentration of Solute in Stationary Phase/Concentration of Solute in Mobile Phase

Change in Boiling Point of Solvent

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

Specific Heat Capacity

Go Specific Heat Capacity = Heat Energy/(Mass*Rise in Temperature)

Vapour Pressure

Go Vapour Pressure of Solution = Mole Fraction of Solvent in Solution*Vapour Pressure of Solvent

Relative Atomic Mass of Element

Go Relative Atomic Mass of an Element = Mass of an Atom/((1/12)*Mass of Carbon-12 atom)

Bond Order

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

Molar Volume

Go Molar Volume = (Atomic Weight*Molar Mass)/Density

Boiling Point

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

Relative Molecular Mass of Compound

Go Relative Molecular Mass = Mass of Molecule/(1/12*Mass of Carbon-12 atom)

Molecular Formula

Go Molecular Formula = Molar Mass/Mass of Empirical Formulas

Percent by Weight

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

Theoretical Yield

Go Theoretical Yield = (Actual Yield/Percent Yield)*100

Determination of Atomic Mass using Dulong and Pettit's method

Go Atomic Mass = 6.4/Specific Heat of Element

Average Atomic Mass Formula

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.

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