The reaction of $[\text{Co}(\text{NH}_3)_5\text{Cl}]\text{Cl}_2$ with excess AgNO$_3$ is as follows:
\[[\text{Co}(\text{NH}_3)_5\text{Cl}]\text{Cl}_2 + \text{excess AgNO}_3 \rightarrow 2\text{AgCl (2 moles)}\]
In the complex $[\text{Co}(\text{NH}_3)_5\text{Cl}]\text{Cl}_2$:
The inner coordination sphere contains 1 Cl ligand.
The outer coordination sphere contains 2 Cl$^-$ ions, which react with AgNO$_3$ to give 2 moles of AgCl.
Let $x$ be the oxidation state of Co. The total charge on the complex is neutral. Therefore:
\[x + 0 \text{ (from 5 NH}_3\text{)} + (-1 \text{ from 1 Cl}) + (-2 \text{ from 2 Cl}^-) = 0\]
\[x - 1 - 2 = 0\]
\[x = +3\]
Here, $n = 5$ (the number of NH$_3$ ligands). Thus:
\[x + n = 3 + 5 = 8\]
Final Answer: $x + n = 8$
Match List - I with List - II:
List - I:
(A) \([ \text{MnBr}_4]^{2-}\)
(B) \([ \text{FeF}_6]^{3-}\)
(C) \([ \text{Co(C}_2\text{O}_4)_3]^{3-}\)
(D) \([ \text{Ni(CO)}_4]\)
List - II:
(I) d²sp³ diamagnetic
(II) sp²d² paramagnetic
(III) sp³ diamagnetic
(IV) sp³ paramagnetic