# 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?

Sep 20, 2016

You have the numerical values to calculate the equilibrium.

#### Explanation:

$2 {H}_{2} \left(g\right) + {S}_{2} \left(g\right) r i g h t \le f t h a r p \infty n s 2 {H}_{2} S \left(g\right)$

${K}_{e q}$ $=$ $\frac{{\left[{H}_{2} S\right]}^{2}}{{\left[{H}_{2}\right]}^{2} \left[{S}_{2}\right]}$ $=$ $\frac{{\left(68.5 \cdot m o l \cdot {L}^{-} 1\right)}^{2}}{{\left(0.50 \cdot m o l \cdot {L}^{-} 1\right)}^{2} \left(0.020 \cdot m o l \cdot {L}^{-} 1\right)}$

$=$ $\text{A large number}$

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