Answer:
[Cl₂] = 0.1804M
Explanation:
The reaction of Si with Cl₂ is:
Si(s) + 2Cl₂(g) ⇄ SiCl₄(g)
Where equilibrium constant, k, is:
k = 0.30 = [SiCl₄] / [Cl₂]²
<em>Si(s) is not in the equilibrium reaction because pure solids don't take part in the equilibrium.</em>
As initial concentration of SiCl₄ is 0.10mol / 1L = 0.10M, when the equilibrium is established, concentrations are:
[SiCl₄] = 0.10M - X
[Cl₂] = 2X
<em>Where X is the reaction coordinate.</em>
Replacing in k equation:
0.30 = [0.10-X] / [2X]²
0.30 = [0.10-X] / 4X²
1.2X² = 0.10 - X
1.2X² + X - 0.10 = 0
<em>Solving for X:</em>
X = - 0.92M → <em>False solution. There is no negative concentrations.</em>
X = 0.0902M → Right solution.
[Cl₂] = 2×0.0902M = 0.1804M
<h3> [Cl₂] = 0.1804M</h3>
Answer:
Answer in explanation
Explanation:
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Answer:
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Hope this helps!