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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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: \[ \operatorname{Cr}(\mathrm{OH})_{3} \]

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The chemical formula for the unknown compound is \(\operatorname{Cr}(\mathrm{OH})_{3}\).
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