Calculate the average atomic mass of iridium. Iridium has two isotopes. Iridium-191 has a mass of 191.0 amu and a percent abundance of 37.58%. Iridium-193 has a mass of 193.0 amu and a percent abundance of 62.42%.

To calculate the average atomic mass of iridium, we can use the following formula:

\[
\text{Average Atomic Mass} = (\text{Fractional Abundance of Isotope 1} \times \text{Mass of Isotope 1}) + (\text{Fractional Abundance of Isotope 2} \times \text{Mass of Isotope 2})
\]

Given:
- Isotope 1: Iridium-191 with a mass of 191.0 amu and a percent abundance of 37.58%.
- Isotope 2: Iridium-193 with a mass of 193.0 amu and a percent abundance of 62.42%.

First, convert the percent abundances to fractional abundances:
- Fractional abundance of Iridium-191 = \( \frac{37.58}{100} = 0.3758 \)
- Fractional abundance of Iridium-193 = \( \frac{62.42}{100} = 0.6242 \)

Now, plug these values into the formula:

\[
\text{Average Atomic Mass} = (0.3758 \times 191.0) + (0.6242 \times 193.0)
\]

Calculate each term:

\[
0.3758 \times 191.0 = 71.7678 \text{ amu}
\]
\[
0.6242 \times 193.0 = 120.4746 \text{ amu}
\]

Finally, add these two results together to find the average atomic mass:

\[
\text{Average Atomic Mass} = 71.7678 + 120.4746 = 192.2424 \text{ amu}
\]

Therefore, the average atomic mass of iridium is approximately **192.24 amu**.

Would you like further details or have any questions?

Here are some related questions to consider:
1. What is the significance of atomic mass in chemical reactions?
2. How does the presence of isotopes affect the average atomic mass of an element?
3. Why do elements have more than one isotope?
4. How are the percent abundances of isotopes determined experimentally?
5. What would the average atomic mass be if one of the isotopes had a significantly higher abundance?

**Tip:** Always ensure that the percent abundances add up to 100% when calculating average atomic mass.

Learn how to calculate the average atomic mass of iridium using the provided isotopic data. This problem covers key concepts such as average atomic mass formula, fractional abundance calculation, and isotope contributions. Suitable for high school students and chemistry enthusiasts.

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