For the reactions system #2H_2(g) + S_2(g) rightleftharpoons 2H_2S(g)#, a 1.00 liter vessel is found to contain 0.50 moles of #H_2# 0.020 moles of #S_2#, and 68,5 moles of #H_2S#. How do you calculate the numerical value of the Keq of this system?

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Answer 1 · 2016-09-20T04:35:42

You have the numerical values to calculate the equilibrium.

#2H_2(g) + S_2(g) rightleftharpoons 2H_2S(g)#

#K_(eq)# #=# #([H_2S]^2)/([H_2]^2[S_2])# #=# #((68.5*mol*L^-1)^2)/((0.50*mol*L^-1)^2(0.020*mol*L^-1))#

#=# #"A large number"#

I don't believe this. Disulfur is an exceptionally high energy molecule, and I do not believe that these figures are authentic.