is 12.5 M
![K_{c}=\frac{[C_{2}H_{5}OH]}{[C_{2}H_{4}][H_{2}O]}](/tpl/images/0540/2224/b68d8.png)
represents equilibrium constant in terms of concentration and species inside third bracket represent equilibrium concentrations![[C_{2}H_{4}]=0.015M](/tpl/images/0540/2224/3b394.png)
, ![[C_{2}H_{5}OH]=1.69M](/tpl/images/0540/2224/5d6f4.png)
and 
![[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](/tpl/images/0540/2224/0a407.png)
Consider the following reaction, equilibrium concentrations, and equilibrium constant at
a par...
Chemistry, 10.03.2020 06:15 enevjordan
Consider the following reaction, equilibrium concentrations, and equilibrium constant at
a particular temperature. Determine the equilibrium concentration of H2O(g): [C2H4]eq = 0.015
M, [C2H5OH]eq = 1.69 M
C2H4(g) + H2O(g) ? C2H5OH(g) Kc = 9.0
Answers: 1
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