ICE tables are used for calculating changes in concentration in an equilibrium system. I represents the initial concentration. C the change in concentration between the initial value and the equilibrium value, and E the final concentration at equilibrium. The equilibrium constant for the following system is 19.9 at 373K. Cl2(g)+F2(g)2ClF(g) The initial concentrations of Cl2,F2, and CIF are 0.20M,0.50M, and 1.5M respectively. Complete the ICE table to show the changes and equilibrium concentrations using the values from the following list. Provide your answer below: \begin{tabular}{|c|c|c|c|} \hline & {[Cl2]} & {[F2]} & {[ClF]} \\ \hline I & & & \\ \hline C & & & \\ \hline E & & & \\ \hline \end{tabular} \begin{tabular}{lll|lllllllll} 0.20 & 0.50 & 1.5 & x & +x & 2x & +2x & 0.20+x & 0.20x & 0.20+2x & 0.202x \\ \hline \end{tabular}