Given #100*g# EACH of carbon disulfide, and chlorine gas, #0.423*mol# carbon tetrachloride results. What is the percentage yield?

1 Answer
Oct 22, 2017

I get #"% yield"-=90%#...........

Explanation:

We need a stoichiometric equation....

#"CS"_2(g) +3"Cl"_2(g) stackrel(MnCl_2"/"AlCl_3)rarr "CCl"_4(g) +S_2"Cl_2(g)#

Note that this reaction SHOULD have been quoted with the question......this is what you are missing.

This is not a reaction I would be very happy to do....sulfide is oxidized to #stackrel(+I)S#, chlorine is reduced to #stackrel(-I)Cl#..and the reaction would pen and ink abominably.

#"Moles of carbon disulfide"=(100*g)/(76.13*g*mol^-1)=1.31*mol#

#"Moles of dichlorine"=(100*g)/(70.9*g*mol^-1)=1.41*mol#

Clearly, dichorine is the reagent in deficiency, and at most #(1.41*mol)/3=0.470*mol# with respect to carbon tet would result.....

We gots....#(65.0*g)/(153.82*g*mol^-1)=0.423*mol#

And so we gots a respectable yield of ......

#(0.423*mol)/(0.470*mol)xx100%=??%#