An element Z contains two naturally occurring isotopes 35Z17 and 37Z17. If the average atomic mass of this element be 35.5 u, calculate the percentage of two isotopes.
Average atomic mass of Z = 35.5u
Let the % of an isotope with mass number 35 be x
Then the % of an isotope with mass number 37 will be 100−x.
Average atomic mass of chlorine = 35$\frac{x}{100}$+37$\frac{100-x}{100}$
35=$\frac{35x}{100}$+$\frac{37(100-x)}{100}$
x=75
Therefore, the % of the isotope 3517Cl is 75 and the % of the isotope 3517Cl is 25.
Related Articles
- (a) What are radioactive isotopes ? Give two examples of radioactive isotopes.(b) Give any two uses of radioactive isotopes.(c) An element Z contains two naturally occurring isotopes 3517Z and 3717Z. If the average atomic mass of this element be 35.5 u, calculate the percentage of two isotopes.
- The average atomic mass of a sample of element X is 16.2 u. What are the percentages of isotopes 168X and 188X in the sample?
- If bromine atom is available in the form of say, two isotopes 7935Br (49.7%) and 8135Br (50.3%), calculate the average atomic mass of bromine atom.
- Explain with examples:(i) Atomic number(ii) Mass number,(iii) Isotopes and(iv) Isobars.Give any two uses of isotopes.
- What is the reason for the different atomic masses of the isotopes of an element?
- Calculate the molecular mass of chloroform(CHCl3).(Atomic masses: C = 12 u; H = 1 u; Cl = 35.5 u)
- Which of the following are the characteristics of isotopes of an element?Isotopes of an element have the same atomic massesIsotopes of an element have the same atomic numberIsotopes of an element show the same physical propertiesIsotopes of an element show the same chemical properties(a) (i), (iii) and (iv)(b) (ii), (iii) and (iv)(c) (ii) and (iii) (d) (ii) and (iv)
- Establish the relationship between atomic number, mass number, isotopes, isobars, and valency of an atom.
- (a) What are radioactive isotopes? Give two examples of radioactive isotopes.(b) Give any two uses of radioactive isotopes.
- The mass of one atom of an element X is 2.0 × 10–23 g.(i) Calculate the atomic mass of element X.(ii) What could element X be?
- What is meant by atomic mass, gram atomic mass of an element? Why is the mass have different expressions i.e., ‘u’ and ‘g’?
- Calculate the number of molecules present in a drop of chloroform (CHCl3) weighing 0.0239 g.(Atomic mass : C = 12 u ; H = 1 u ; Cl = 35.5 u)
- An element X has a mass number 4 and atomic number 2. Write the valency of this element?
- The atomic masses of three elements X, Y and Z having similar chemical properties are 7, 23 and 39 respectively.(a) Calculate the average atomic mass of elements X and Z. (b) How does the average atomic mass of elements X and Z compare with the atomic mass of element Y? (c) Which law of classification of elements is illustrated by this example? (d) What could the elements X, Y and Z be? (e) Give another example of a set of elements which can be classified according to this law.
- If one gram of sulphur contains x atoms, calculate the number of atoms in one gram of oxygen element.(Atomic masses : S = 32 u ; O = 16 u)
Kickstart Your Career
Get certified by completing the course
Get Started
Data Structure
Networking
RDBMS
Operating System
Java
MS Excel
iOS
HTML
CSS
Android
Python
C Programming
C++
C#
MongoDB
MySQL
Javascript
PHP
Physics
Chemistry
Biology
Mathematics
English
Economics
Psychology
Social Studies
Fashion Studies
Legal Studies