An element has two main isotopes of mass numbers $85$ and $87$. In nature,they occur in the ratio of $75\%$ and $25\%$ respectively. The atomic weight of the element will be approximately:
- A$86$
- B$86.5$
- C$85.5$
- D$85.75$
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Use the data given in the following table to calculate the molar mass of naturally occurring argon isotopes:
Isotope Isotopic molar mass $(g \, mol^{-1})$ Abundance (%) $^{36}Ar$ $35.96755$ $0.337$ $^{38}Ar$ $37.96272$ $0.063$ $^{40}Ar$ $39.9624$ $99.600$
| Isotope | Isotopic molar mass $(g \, mol^{-1})$ | Abundance (%) |
| $^{36}Ar$ | $35.96755$ | $0.337$ |
| $^{38}Ar$ | $37.96272$ | $0.063$ |
| $^{40}Ar$ | $39.9624$ | $99.600$ |
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