`K_(p)=0.04 atm` at `899 K` for the equilibrium shown below. What is the equilibrium concentration of `C_(2)H_(6)` when it is placed in a flask at `4.0 atm` pressure and allowed to come to equilibrium?
`C_(2)H_(6)(g) hArr C_(2)H_(4)(g)+H_(2)(g)`

Explanation

To solve the problem, we need to find the equilibrium concentration of \( C_2H_6 \) when it is placed in a flask at a pressure of \( 4.0 \, \text{atm} \) and allowed to come to equilibrium. We are given that \( K_p = 0.04 \, \text{atm} \) at \( 899 \, \text{K} \) for the reaction:

\[ C_2H_6(g) \rightleftharpoons C_2H_4(g) + H_2(g) \]

### Step-by-Step Solution:

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