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Type the correct answer in the box. Round your answer to the nearest hundredth.

Element X has two isotopes. The table gives information about these isotopes.

[tex]\[
\begin{tabular}{|c|c|c|}
\hline
Isotope & \begin{tabular}{c}
Atomic \\
Mass (amu)
\end{tabular} & \begin{tabular}{c}
Abundance \\
(\%)
\end{tabular} \\
\hline
X-63 & 62.9296 & 69.15 \\
\hline
X-65 & 64.9278 & 30.85 \\
\hline
\end{tabular}
\][/tex]

The average atomic mass of element X is [tex]$\square$[/tex] amu.

Sagot :

GinnyAnsweridn
To find the average atomic mass of element X given the data for its two isotopes, we follow these steps:

1. Identify the mass and abundance of each isotope:
- The atomic mass of isotope X-63 is 62.9296 amu.
- The abundance of isotope X-63 is 69.15%.
- The atomic mass of isotope X-65 is 64.9278 amu.
- The abundance of isotope X-65 is 30.85%.

2. Convert the abundance percentages into decimal fractions:
- The abundance of isotope X-63 as a fraction is [tex]\( 69.15\% \)[/tex] or [tex]\( 0.6915 \)[/tex].
- The abundance of isotope X-65 as a fraction is [tex]\( 30.85\% \)[/tex] or [tex]\( 0.3085 \)[/tex].

3. Calculate the weighted average of the atomic masses:
- Multiply the atomic mass of each isotope by its respective fraction.
- For isotope X-63: [tex]\( 62.9296 \times 0.6915 \)[/tex].
- For isotope X-65: [tex]\( 64.9278 \times 0.3085 \)[/tex].

4. Sum the weighted masses to find the average atomic mass:
- Average atomic mass = [tex]\( (62.9296 \times 0.6915) + (64.9278 \times 0.3085) \)[/tex].

5. Round the result to the nearest hundredth:
- After performing the calculations and summing the results, we obtain an average atomic mass of 63.55 amu.

Therefore, the average atomic mass of element X is [tex]\( \boxed{63.55} \)[/tex] amu.
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