a)
According to the following reaction, how many moles of bromine trifluoride are necessary to form 0.841 moles fluorine gas?
bromine trifluoride (g) →bromine(g) + fluorine(g)
_______moles bromine trifluoride
b) According to the following reaction, how
many moles of dichloromethane
(CH2Cl2) will be formed upon the
complete reaction of 0.227 moles methane
(CH4) with excess carbon
tetrachloride?
methane (CH4) (g) +carbon tetrachloride (g)→dichloromethane
(CH2Cl2) (g)
________moles dichloromethane
(CH2Cl2)
(a) from the balanced equation we see that
2 moles of BrF3 gives 3 moles of Fluorine gas
So 0.841 moles of Fluorine gas will be given by 2/3* 0.841 moles of BrF3 = 0.56 moles of boron trifluoride.
(b) 1 mole of methane forms 2 moles of dichloromethane
So 0.227 moles of CH4 will form 2/1*0.227= 0.454 moles of.dichloromethane.
According to the following reaction, how many moles of bromine trifluoride are necessary to form 0.841 moles fluorine gas?
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For this reaction, 2.79 g methane (CH4) reacts with 30.0 g carbon tetrachloride. methane (CH4) (g) + carbon tetrachloride (g) dichloromethane (CH2Cl2) (g) What is the maximum mass of dichloromethane (CH2Cl2) that can be formed? g What is the FORMULA for the limiting reagent? What mass of the excess reagent remains after the reaction is complete? g
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