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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?

Answer 1

Ellie Andrews

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"#

Given that sulfur is a molecule with extraordinarily high energy, I don't think these numbers are accurate.

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Answer 2

Noah Aldrich

[ K_{\text{eq}} = \frac{{[\text{H}_2S]^2}}{{[\text{H}_2]^2[\text{S}_2]}} ]

[ K_{\text{eq}} = \frac{{(68.5)^2}}{{(0.50)^2(0.020)}} ]

[ K_{\text{eq}} \approx 9.4 \times 10^5 ]

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.