The `K_(c)` for `A_(2(g))+B_(2(g))hArr2AB_((g))` at `100^(@)C` is `50`. If one litre flasks containing one mole of `A_(2)` is connected with a two litre flask containing `2 "mole"` of `B_(2)`, how many mole of `AB` will be formed at `100 ^(@)C`?

Explanation

To solve the problem step by step, we will follow the equilibrium concepts and calculations based on the provided reaction and the equilibrium constant \( K_c \).

### Step 1: Write the balanced chemical equation
The balanced chemical equation for the reaction is:
\[ A_2(g) + B_2(g) \rightleftharpoons 2AB(g) \]

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