A beaker contains nickel(ii sulfate, zinc(ii sulfate and solid iron. what species in this beaker will be reduced?
2 answers:
Answer:
Nickel (II) to solid nickel.
Explanation:
Hello,
In this case, the placed species are nickel (II) sulfate , zinc sulfate
and solid iron
. Now, as the nickel sulfate is more reactive than the zinc sulfate, it will experience the following reduction half-reaction from nickel (II) to solid nickel:
Nevertheless, it is possible that the zinc might experience the same reduction reaction from zinc (II) to solid zinc as well.
Best regards.
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The equilibrium constant of a reaction is defined as:
"The ratio between equilibrium concentrations of products powered to their reaction quotient and equilibrium concentration of reactants powered to thier reaction quotient".
The reaction quotient, Q, has the same algebraic expressions but use the actual concentrations of reactants.
To solve this question we need this additional information:
<em>For this reaction, K = 6.0x10⁻² and the initial concentrations of the reactants are:</em>
<em>[N₂] = 4.0M; [NH₃] = 1.0x10⁻⁴M and [H₂] = 1.0x10⁻²M</em>
<em />
Thus, for the reaction:
N₂ + 3H₂ ⇄ 2NH₃
The equilibrium constant, K, of this reaction, is defined as:
And Q, is:
Where actual concentrations are:
[NH₃] = 1.0x10⁻⁴M
[N₂] = 4.0M
[H₂] = 2.5x10⁻¹M
Replacing:
As Q < K,
<h3>The chemical system will shift to the right in order to produce more NH₃</h3>Learn more about chemical equililbrium in: