Barker Klein
08/03/2023 · Middle School
An unknown compound has the following chemical formula: \[ \operatorname{Cr}(\mathrm{OH})_{\mathrm{x}} \] where \( x \) stands for a whole number. Measurements also show that a certain sample of the unknown compound contains 7.90 mol of oxygen and 2.63 mol of chromium. Write the complete chemical formula for the unknown compound.
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Step-by-step Solution
To determine the complete chemical formula for the unknown compound \(\operatorname{Cr}(\mathrm{OH})_{\mathrm{x}}\), we need to find the value of \(x\).
The formula \(\operatorname{Cr}(\mathrm{OH})_{\mathrm{x}}\) indicates that each chromium (Cr) atom is associated with \(x\) hydroxide (OH) groups. Each hydroxide group contains one oxygen atom and one hydrogen atom.
From the information provided:
- The sample contains 7.90 mol of oxygen.
- The sample contains 2.63 mol of chromium.
Since each hydroxide group contributes one oxygen atom, the total number of oxygen atoms in the compound can be expressed as:
\[
\text{Total oxygen} = x \times \text{moles of Cr}
\]
Substituting the known values:
\[
7.90 \, \text{mol} = x \times 2.63 \, \text{mol}
\]
Now, we can solve for \(x\):
\[
x = \frac{7.90 \, \text{mol}}{2.63 \, \text{mol}} \approx 3.00
\]
Since \(x\) must be a whole number, we round \(3.00\) to \(3\).
Thus, the complete chemical formula for the unknown compound is:
\[
\operatorname{Cr}(\mathrm{OH})_{3}
\]
Quick Answer
The chemical formula for the unknown compound is \(\operatorname{Cr}(\mathrm{OH})_{3}\).
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