QQuestionChemistry
QuestionChemistry
Calculate the number of oxygen atoms in a 110.0 g sample of forsterite (Mg^2 SiO 4 ).
Be sure your answer has a unit symbol if necessary, and round it to 4 significant digits.
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Answer
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Step 1: Find the molar mass of forsterite (Mg^2 SiO4)
The molar mass of a compound is the sum of the molar masses of its constituent elements. The molar masses of Mg, Si, and O are 24.305 g/mol, 28.086 g/mol, and 15.9994 g/mol, respectively. Molar mass of Mg^2SiO^4 = 2 * Molar mass of Mg + Molar mass of Si + 4 * Molar mass of O \begin{align*} &= 2 \times 24.305~\text{g/mol} + 28.086~\text{g/mol} + 4 \times 15.9994~\text{g/mol} \ &= 72.91~\text{g/mol} + 28.086~\text{g/mol} + 63.9976~\text{g/mol} \ &= 165.0036~\text{g/mol} \end{align*}
Step 2: Calculate the number of moles in the sample
To find the number of moles (n) in 110.0 g of forsterite, divide the mass of the sample by its molar mass.
Final Answer
The number of oxygen atoms in a 110.0 g sample of forsterite is approximately 2.668 mol (42.60 g).
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