Question

A mixture containing C₂H₅Cl, HCl, C₂H₆, and Cl₂, all at an initial partial pressure of 1.27 atm, is allowed to achieve equilibrium according to the equation below. At equilibrium, the partial pressure of Cl₂ is observed to have increased by 0.11 atm. Determine K_p for this chemical equilibrium. Report your answer to 3 significant figures in scientific notation.

Answer 1

Assuming the equation is;

$C_2H_{6(g)}+Cl_{2(g)}\to\>C_2H_5Cl_{(g)}+HCl_{(g)}$

$\begin{matrix} &C_2H_6&Cl_2&CH_2H_5Cl & HCl \\ I& 1.27&1.27&1.27&1.27\\ C&0.11&0.11&-0.11&-0.11\\ E&1.38&1.38&1.16&1.16 \end{matrix}$

$K_p=\frac{1.16×1.16}{1.38×1.38}=7.07×10^{-1}$