For the following reaction, equilibrium constant `K_(c)` at 298 K is `1.6xx10^(17)`
`Fe_((aq))^(2+)+S_((aq))^(2) hArr FeS(s)`
When equal volume of 0.06 `M Fe^(2+)` and 0.2 `Ms^(-2)` solution are mixed, then equilibrium concentration of `Fe^(2+)` is found to be `Yxx10^(-17) M`. Y is

Explanation

To solve the problem step by step, we will follow these steps:

### Step 1: Understand the Reaction and Initial Concentrations
The reaction given is:
\[ \text{Fe}^{2+} + \text{S}^{2-} \rightleftharpoons \text{FeS (s)} \]
The equilibrium constant \( K_c \) at 298 K is \( 1.6 \times 10^{17} \).

We have:
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