Gracexoxdyer
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#1
Report Thread starter 3 years ago
#1
Fluorine reacts with sulfur to produce sulfur hexafluoride (SF_6)

S + 3F_2 —> SF_6

Relative formula masses, M_r: F_2 = 38. SF_6 =146

Calculate the mass of sulfur hexafluoride produced when 0.950g of fluorine is reacted with an excess of sulfur.

Give your answer to 3 significant figures
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username3385296
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#2
Report 3 years ago
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Calculate the number of moles of F2 by doing mass/Mr - this is the limiting reagent. Since the mole ratio of F2 to SF6 is 3:1, meaning in an excess of sulfur that 3 moles of fluorine would react with 1 mole of sulfur to produce 1 mole of SF6, the moles of sulfur hexafluoride produced is the moles of fluorine calculated divided by 3. The mass of sulfur hexafluoride produced is then the Mr of sodium hexafluoride multiplied by the moles of sulfur hexafluoride. Hope that helps!
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