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Natural chlorine is composed of two isot...

Natural chlorine is composed of two isotopes `""_(17)Cl^(35)` and `""_(17)Cl^(37)` with masses 34.968 and 36.968, respectively. If their relative abundance are 75.18% and 24.22% respectively, calculate the composite atomic mass of the natural chlorine.

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To calculate the composite atomic mass of natural chlorine, we will use the formula for the weighted average of the isotopes based on their relative abundances. ### Step-by-Step Solution: 1. **Identify the isotopes and their masses:** - Isotope 1: \( ^{35}\text{Cl} \) with mass \( m_1 = 34.968 \, \text{u} \) - Isotope 2: \( ^{37}\text{Cl} \) with mass \( m_2 = 36.968 \, \text{u} \) ...
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Natural Chlorine is found to be a mixutre of two isotopes of masses 34.98 a.m.u and 36.98 a.m.u. respectively. Their relative abundances are 75.4 and 24.6% respectively. Find the composite atomic mass of natural chlorine.

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Knowledge Check

  • Chlorine has two isotopes having masses 34.98 u and 36.98 u with relative abundance of 75.4% and 24.6% ,respectively. The average atomic mass of chlorine is

    A
    34.98
    B
    36.98
    C
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    D
    35

  • The relative abundance of two isotopes of atomic masses 85 and 87 are 75% and 25% respectively. The average atomic mass of element is:

    A
    86
    B
    40
    C
    85.5
    D
    75.5

  • Oxygen occurs in nature as a mixture of isotopes ""^16O, ""^17O " and " ""^18O having masses of 15.995 u, 16.999 u and 17.999 u and relative abundance of 99.763%, 0.037% and 0.0200% respectively. What is the average atomic mass of oxygen?

    A
    15.999 u
    B
    16.999 u
    C
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    D
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    Natural chlorine consists of two isotopes : 75% ""_(17)^(35)Cl and 25% ""_(17)^(37)Cl . Calculate the average atomic mass of chlorine .

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