Home
Class 11
CHEMISTRY
Calculate the atomic mass (average) of c...

Calculate the atomic mass (average) of chlorine using the following data:
`{:(,,"% natural abundance",,"Molar mass"),(.^(35)Cl,,75.77,,34.9689),(.^(37)Cl,,24.23,,36.9659):}`

Text Solution

AI Generated Solution

To calculate the average atomic mass of chlorine using the provided data, we will follow these steps: ### Step 1: Understand the Data We have two isotopes of chlorine: - \(^{35}Cl\) with a natural abundance of 75.77% and a molar mass of 34.9689 g/mol. - \(^{37}Cl\) with a natural abundance of 24.23% and a molar mass of 36.9659 g/mol. ### Step 2: Convert Percentages to Fractions ...
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • REDOX REACTIONS

    NCERT ENGLISH|Exercise EXERCISE|30 Videos

  • STATES OF MATTER

    NCERT ENGLISH|Exercise EXERCISE|23 Videos

Similar Questions

Explore conceptually related problems

Calculate the average atomic mass of hydrogen using the following data Isotope % Natural abundance Molar mass .^(1)H 99.985 1 .^(2)H 0.015 2

Average atomic mass of chlorine is 35.5 then the correct naturally occuring molar ratio of "^(35)Cl & ^(37)Cl is

Average atomic mass of chlorine is 35.5 then the correct naturally occuring molar ratio of "^(35)Cl & ^(37)Cl is

Use data given in the following table to calculate the molar mass of naturaly occuring argon isotopes: {:("Isotope",,"Isotopic molar mass",,"Abundance"),(.^(36)Ar,,35.96755 g mol^(-1),,0.337%),(.^(38)Ar,,37.96272 g mol^(-1),,0.063%),(.^(40)Ar,,39.9624 g mol^(-1),,99.600%):} (Round of the answer to the nearest whole number ).

Use data given in the following table to calculate the molar mass of naturaly occuring argon isotopes: {:("Isotope",,"Isotopic molar mass",,"Abundance"),(.^(36)Ar,,35.96755 g mol^(-1),,0.337%),(.^(38)Ar,,37.96272 g mol^(-1),,0.063%),(.^(40)Ar,,39.9624 g mol^(-1),,99.600%):}

In a periodic table, the average atomic mass of magnesium is given as 24.312 u . The average value is based on their relative natural abundance on earth. The three isotopes and their masses are ._12Mg^(24) (23.98504u) , ._(12)Mg^(25) (24.98584) and ._12Mg^(26) (25.98259 u) . The natural abundance of ._12Mg^(24) is 78.99% by mass. Calculate the abundances of the other two isotopes.

A Polydisperse mixture of a polymer can be describe by the following composition-molar mass data: {:(Mass%),25.0,50.0,25.0),(Mi(kgmol^(-1)),1.00,1.20,1.40):} Calculate the number -average.

Calculate the relative molecular masses (or molecular weights), of the following compounds : Urea, NH_(2)CONH_(2) (Given : Atomic mass in amu of N = 14, H = 1, S = 32, O = 16, C = 12, Pt= 195, Cl= 35.5, Cu= 63.5)

The force with which the erth attracts an object is called the weight of the object. Calculate the weight of the moon from the following data: The universal constant of gravitastion G=6.67xx10^-11 N-m^2/kg^2 mass of the moon =7.36xx10^22 kg, mass of the earth =6xx10^24 kg and the distasnce between the earth and the moon=3.8xx10^5 km.

Calculate the empirical formula of a compound having following - percentage composition. Carbon = 25.41%, hydrogen 3.17%, oxygen = 33.86% and chlorine 37.56%.[C = 12 , H = 1 , O = 16 , Cl = 35.5)

Home
Profile