Consider this chemical reaction: #H_2(g) + I_2(g) rightleftharpoons 2HI(g)#. At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.15 M, 0.033 M, and 0.55 M, respectively. What is the value of #K_(eq)# for this reaction?

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Answer 1 · 2016-12-01T10:28:06

#K_"eq">50#

For the reaction:

#H_2(g) + I_2(g) rightleftharpoons2HI(g)#

#K_"eq"=[HI(g)]^2/([H_2(g)][I_2(g)])#

#=# #(0.55*mol*L^-1)^2/(0.15*mol*L^-1xx0.033*mol*L^-1)#

#=# #??#