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Sagot :
Thus one concludes that the answer is S2F10, the molecular formula of SxFy. There are five compounds in the family of sulfur–fluorine compounds with the general formula SxFy.
The empirical formula must be SF5, according to a typical analysis. S2F10 is the most likely candidate as a result. S2F10 has a 254 g molar mass. So,.0955 g is equal to.000376 moles. The ideal gas law (PV = nRT) can be used with n =.000376, V =.089 L, and T = 318K to calculate the pressure if it is assumed that S2F10 would be in the gas phase at 45C. The outcome is roughly.11 atm, or 83.6 mmHg. Nearly 83.8 is where this comes in. Thus, it is determined that the response is S2F10. The empirical formula's conventional analysis is as follows: Consider a sample of 100 g. The sample's Sulfur content would be 25.23 g as the%S is 25.23. Given that S has a molar mass of 32, this is .788 mole S. The remaining 74.8 g is F. Since the molar mass of F is 19, this is 3.93 moles F. The ratio 3.93 / .788 ~ 5 , so the empirical formula is SF5. An molecule with an odd number of F would have an unpaired electron - not likely.
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