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A compound of silicon and fluorine was analyzed and found to consist of 33.0% silicon and 67.0% fluorine by mass. The molecular mass of the compound was determined by experiment to be 170 g/mol. What is the molecular formula of the compound? (Si2F6)
We first compute the no. of moles of each element in the compound. So first, the Si is said to have 33% by mass in the solution. So we solve: (0.33 g Si/1 g sol'n)(1 mol Si/28 g Si)(170 g sol'n/1 mol sol'n) = 2.00 moles of Si. Then next we solve for the moles of F. We follow the same procedure: (0.67 g F/1 g sol'n)(1 mol F/19 g F)(170 g sol'n/1 mol sol'n) = 5.99 or 6.00 moles of F. So we have Si2F6.
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