QQuestionGeology
QuestionGeology
Calculate the number of oxygen atoms in a
110.0g
sample of forsterite
Mg^2SiO^4
.
Be sure your answer has a unit symbol if necessary, and round it to
4
significant digits
5 months agoReport content
Answer
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Step 1: Find the molar mass of forsterite (Mg^2SiO4)
Forsterite is made up of the following elements: Magnesium (Mg), Silicon (Si), and Oxygen (O). To find the molar mass of forsterite, we need to sum the atomic masses of each element in one mole of the compound. The atomic masses are as follows: - Mg: 24.305 amu - Si: 28.085 amu - O: 15.999 amu In the formula Mg^2SiO^4, there are 2 magnesium atoms, 1 silicon atom, and 4 oxygen atoms. So the molar mass of forsterite is: Molar mass of forsterite = 2 * Mg + 1 * Si + 4 * O Molar mass of forsterite = 2 * 24.305 amu + 1 * 28.085 amu + 4 * 15.999 amu Molar mass of forsterite ≈ 110.99 g/mol
Step 2: Convert the mass of forsterite to moles
Now, we want to convert the given mass of forsterite (110.0 g) to moles. To do this, divide the mass by the molar mass (calculated in Step 1). Number of moles = mass / molar mass Number of moles = 110.0 g / 110.99 g/mol ≈ 0.990 mol
Final Answer
Approximately 3.96 mol of oxygen atoms are present in a 110.0 g sample of forsterite (Mg^2SiO4).
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