Answer:
[S₂] = 1.27×10⁻⁷ M
Step-by-step explanation:
2 H₂S(g) ⇄ 2 H₂(g) + S₂(g), Kc=1,625x10⁻⁷
The equation of this reaction is:
1,625x10⁻⁷ =
![([H_2]^2[S_2])/([H_(2)S]^2)](https://img.qammunity.org/2020/formulas/chemistry/college/zu46i8r1wtf03c17ceks1ga9akep73mqj1.png)
The equilibrium concentrations are:
[H₂S] = 0,162 - 2x
[H₂] = 0,184 + 2x
[S₂] = x
Replacing:
1,625x10⁻⁷ =
![([0,184+2x]^2[x])/([0,162-2x]^2)](https://img.qammunity.org/2020/formulas/chemistry/college/j576tf7piexkdiq2s2pmc4nt1fr5d3k0a5.png)
Solving:
4x³ + 0,736x² + 0,033856x - 4,3x10⁻⁹
x = 1.27×10⁻⁷
Thus, concentration of S₂ is:
[S₂] = 1.27×10⁻⁷ M