Answer :
Answer:
23000 mg
Explanation:
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Answer:
Answer
Explanation:
To determine the percentage of isotopes 25Mg and 27Mg present in nature, we will use the information provided about the isotopic abundance and the relative atomic mass of magnesium (Mg).
Given:
- Isotopic abundance of 23Mg: 78.70%
- Relative atomic mass (Ar) of Mg: 23.649 g/mol
Let's denote:
- Abundance of 23Mg as \( x \)
- Abundance of 25Mg as \( y \)
- Abundance of 27Mg as \( z \)
The sum of all isotopic abundances should equal 100%, so we have the equation:
\[ x + y + z = 100 \]
We know from the problem statement that the abundance of 23Mg is 78.70%, hence:
\[ x = 78.70 \]
Now, we can express the relative atomic mass (Ar) of magnesium as a weighted average of the isotopes:
\[ \text{Ar} = x \cdot \text{Ar}(23\text{Mg}) + y \cdot \text{Ar}(25\text{Mg}) + z \cdot \text{Ar}(27\text{Mg}) \]
Substituting the values:
\[ 23.649 = 78.70 \times 23 + y \times 25 + z \times 27 \]
Now, solve for \( y \) and \( z \):
1. Calculate \( y + z \):
\[ y + z = 100 - x = 100 - 78.70 = 21.30 \]
2. Substitute \( y + z \) into the equation:
\[ 23.649 = 78.70 \times 23