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------------------------------------------------ Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of [tex]H_2O(g)[/tex]:

- [tex][C_2H_4]_{eq} = 0.015 \, M[/tex]
- [tex][C_2H_5OH]_{eq} = 1.69 \, M[/tex]

\[C_2H_4(g) + H_2O(g) \rightleftharpoons C_2H_5OH(g)\]

\[K_c = 9.0\]

Answer :

Answer:

Equilibrium concentration of [tex]H_{2}O[/tex] is 12.5 M

Explanation:

Given reaction: [tex]C_{2}H_{4}+H_{2}O\rightleftharpoons C_{2}H_{5}OH[/tex]

Here, [tex]K_{c}=\frac{[C_{2}H_{5}OH]}{[C_{2}H_{4}][H_{2}O]}[/tex]

where [tex]K_{c}[/tex] represents equilibrium constant in terms of concentration and species inside third bracket represent equilibrium concentrations

Here, [tex][C_{2}H_{4}]=0.015M[/tex] , [tex][C_{2}H_{5}OH]=1.69M[/tex] and [tex]K_{c}=9.0[/tex]

So, [tex][H_{2}O]=\frac{[C_{2}H_{5}OH]}{[C_{2}H_{4}]\times K_{c}}=\frac{1.69}{0.015\times 9.0}=12.5M[/tex]

Hence equilibrium concentration of [tex]H_{2}O[/tex] is 12.5 M

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