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In a nuclear reaction, which of the following must be conserved?
1 answer:
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Answer:
Here's what I get
Explanation:
You have an equilibrium reaction between Fe³⁺/ SCN⁻ and FeSCN²⁺.
When you add AgNO₃, the Ag⁺ reacts with the SCN⁻. It forms a colourless precipitate of Ag(SCN).
Ag⁺(aq) + SCN⁻(aq) ⟶ AcSCN(s)
According to Le Châtelier's Principle, when we apply a stress to a system at equilibrium, the system will respond in a way that tends to relieve the stress.
If you add Ag⁺ to the equilibrium solution, it removes the SCN⁻ [as an Ag(SCN) precipitate].
The system responds by trying to replace the missing SCN⁻:
The Fe(SCN)²⁺ dissociates to form SCN⁻, so the position of equilibrium shifts to the left,
You now have more Fe³⁺ and SCN⁻ and less of the highly coloured Fe(SCN)²⁺ at the new equilibrium.
The deep red colour becomes less intense.