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Old Mar 7th 2017, 06:22 AM   #1
blondeface03
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Theoretical Yield Ni + 2HCl yields NiCl2 + H2

Hey All,

I have the balanced equation of Ni (s) + 2 HCl (aq) -> NiCl2 (aq) + H2 (g)

A.) If 12.0 moles of HCl were reacted, how many moles of Ni would be needed such that there was no excess?

B.) What is the theoretical yield (in grams) of NiCl2 from reacting 12.0 mol HCl?

C.) If 12.0 mol of HCl was reacted and the percent yield of the reaction was 78.5%, what was the actual yield (grams) of NiCl2?

I am completely lost when it comes to theoretical yield questions.. Any help is gladly needed! Thank-you!
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Old Mar 16th 2017, 02:03 AM   #2
MatthijsM
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a) this would be 6 mole
b) there will be 6 mole of NiCl2 if you assume the reaction has a percent yield of 100%
If yes, you just multiply the 6 mole with the moleculair mass of NiCL2.
c) Just multiply answer b) with 0.785 and you get the yield of NiCl2.

If you need a more detailled explination you can message me.
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