If `1.0 "mole"` of `I_(2)` is introduced in a `1.0 litre` flask at `1000 K(K_(c)=10^(-6))`, which one is correct?

Options

A. `[I_(2(g))]gt[I_((g))^(-)]`
B. `[I_(2(g))]lt[I_((g))^(-)]`
C. `[I_(2(g))]=[I_((g))^(-)]`
D. `[I_(2(g))]=1//2[I_((g))^(-)]`

Explanation

To solve the problem, we need to analyze the dissociation of iodine (I₂) in a 1.0 liter flask at 1000 K, where the equilibrium constant \( K_c \) is given as \( 10^{-6} \).

### Step-by-Step Solution:

1. **Write the Dissociation Reaction**:
The dissociation of iodine can be represented as:
\[
I_2 \rightleftharpoons 2I
...