- Average atomic mass is calculated as the weighted average of the masses of its isotopes based on their relative abundance. - The sample contains isotopes with masses 16 u and 18 u in a proportion of 3:1. - This means out of 4 parts, 3 parts have mass 16 u and 1 part has mass 18 u. - Relative abundance of 16u isotope = 3 / (3+1) = 3/4 = 0.75 - Relative abundance of 18u isotope = 1 / (3+1) = 1/4 = 0.25 - Average atomic mass = (Mass₁ × Abundance₁) + (Mass₂ × Abundance₂) - Average atomic mass = (16
A sample of oxygen contains two isotopes of oxygen with masses 16 u and 18 u respectively. The proportion of these isotopes in the sample is 3 : 1. What will be the average atomic mass of oxygen in this sample?
Asked in UPSC NDA 2 2018 · Topic: Atomic Structure (Isotopes, Isobars, and Isotones)
More Chemistry questions
- Atomic mass of an element is equal to the sum of number of
- Chlorine occurs in nature in two isotopic forms of masses 35 u and 37 u in the ratio of 3 : 1 respectively. What is the average atomic mass of the Chlorine atom ?
- For Aluminium (Al) (atomic number : 13, mass number : 27), which one among the following statements is NOT correct ?
- Isotopes are atoms of the same element with different number of
- ₁H³ and ₂He⁴ are
- What are isotopes?
- With reference to the isotopes of elements, consider the following statements :
- The heaviest element known up till January 2015 has the atomic number :