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 Kp for this chemical equilibrium. Report your answer to 3 significant figures in scientific notation.
Assuming the equation is;
"C_2H_{6(g)}+Cl_{2(g)}\\to\\>C_2H_5Cl_{(g)}+HCl_{(g)}"
"\\begin{matrix}\n &C_2H_6&Cl_2&CH_2H_5Cl & HCl \\\\\n I& 1.27&1.27&1.27&1.27\\\\\nC&0.11&0.11&-0.11&-0.11\\\\\nE&1.38&1.38&1.16&1.16\n\\end{matrix}"
"K_p=\\frac{1.16\u00d71.16}{1.38\u00d71.38}=7.07\u00d710^{-1}"
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