Home
Class 12
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

Verified by Experts

Fractional abundance of `.^(35)Cl = 0.7577`, Molar mass = 34.9689
Fractional abundance of `.^(37)Cl = 0.2423`, Molar mass = 36.9659Average atomic mass = (0.7577) (34.9689 amu) + (0.2423) (36.9659 amu)
= 26.4959 + 8.9568 = 35.4527
Promotional Banner

Topper's Solved these Questions

  • STOICHIOMETRY - I

    VMC MODULES ENGLISH|Exercise Level -0 (Long Answer Type)|7 Videos

  • STOICHIOMETRY - I

    VMC MODULES ENGLISH|Exercise Level - 1|75 Videos

  • STOICHIOMETRY - I

    VMC MODULES ENGLISH|Exercise (Level - 0 (Short Answer Type - I)|7 Videos

  • STATES OF MATTER

    VMC MODULES ENGLISH|Exercise IN-CHAPTER EXERCISE-I|10 Videos

  • STOICHIOMETRY-II

    VMC MODULES ENGLISH|Exercise JEE Advanced (Archive)|43 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%):}

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)

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.

Silicon (Si = 28) forms a compound with chlorine (Cl = 35.5) in which 5.6 g of silicon is combined with 21.3 g of chlorine. Calculate the empirical formula of the compound. [Hint. Total mass of silicon and chlorine in the compound = 5.6 + 21.3 = 26.9 % age of Si =(5.6)/(26.9)xx100 and %age of Cl =(21.3)/(26.9)xx100

Calculate the mass of lead chloride formed by treating an aqueous solution 13.24 g of lead nitrate with excess of hydrochloric acid. (Pb = 207, Cl = 35.5, H = 1, O = 16)

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.