(Solved): Predict the equilibrium concentration of CO2 in the reaction described below (for which Kc=5.1 ...

Predict the equilibrium concentration of ${\mathrm{CO}}_2$ in the reaction described below (for which $\mathrm{Kc}=5.1$ at $700\mathrm{K}$ ) by constructing an equilibrium expression for $\mathrm{Qc}$, constructing an ICE table, writing an equilibrium expression for ${\mathrm{Kc}}_{\mathrm{c}}$, and solving for the equilibrium concentration. Complete Parts 1-4 before submitting your answer. $\mathrm{CO}(\mathrm{g})+{\mathrm{H}}_2\mathrm{O}(\mathrm{g})\rightleftharpoons {\mathrm{CO}}_2(\mathrm{g})+{\mathrm{H}}_2(\mathrm{g})$ Based on the initial concentrations and your value of $Q_c$ (Part 1), fill in the ICE table with the appropriate value for each involved species to determine the concentrations of all reactants and products. Predict the equilibrium concentration of ${\mathrm{CO}}_2$ in the reaction described below (for which ${\mathrm{Kc}}_{\mathrm{c}}=5.1$ at $700\mathrm{K}$ ) by constructing an equilibrium expression for $\mathrm{Qc}$, constructing an ICE table, writing an equilibrium expression for $\mathrm{Kc}$, and solving for the equilibrium concentration. Complete Parts $1-4$ before submitting your answer. $\mathrm{CO}(\mathrm{g})+{\mathrm{H}}_2\mathrm{O}(\mathrm{g})\rightleftharpoons {\mathrm{CO}}_2(\mathrm{g})+{\mathrm{H}}_2(\mathrm{g})$ In a $2.0\mathrm{L}$ container at $700\mathrm{K},0.13\mathrm{mol}\mathrm{CO},0.56\mathrm{mol}{\mathrm{H}}_2,{\mathrm{O}}_{1}1.62\mathrm{mol}{\mathrm{CO}}_2$, and $0.43\mathrm{mol}{\mathrm{H}}_2$ are allowed to react. Set up the expression for Qc. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Qc to determine the direction of the reaction. $Q_c=$ Predict the equilibrium concentration of ${\mathrm{CO}}_2$ in the reaction described below (for which $\mathrm{Kc}=5.1$ at $700\mathrm{K}$ ) by constructing an equilibrium expression for ${\mathrm{Qc}}^2$, constructing an ICE table, writing an equilibrium expression for $\mathrm{Kc}$, and solving for the equilibrium concentration. Complete Parts $1-4$ before submitting your answer. $\mathrm{CO}(\mathrm{g})+{\mathrm{H}}_2\mathrm{O}(\mathrm{g})\rightleftharpoons {\mathrm{CO}}_2(\mathrm{g})+{\mathrm{H}}_2(\mathrm{g})$ PREV 1 2 3 4 sed on the information from your ICE Table (Part 2) and the ${\mathrm{Kc}}_{\mathrm{c}}$ expression (Part 3), solve for the equilibrium concentration of ${\mathrm{CO}}_2$. ${\left[{\mathrm{CO}}_2\right]}_{\mathrm{eq}}=M$ Predict the equilibrium concentration of ${\mathrm{CO}}_2$ in the reaction described below (for which $\mathrm{Kc}=5.1$ at $700\mathrm{K}$ ) by constructing an equilibrium expression for $\mathrm{Qc}$, constructing an ICE table, writing an equilibrium expression for $\mathrm{Kc}$, and solving for the equilibrium concentration. Complete Parts 1-4 before submitting your answer. $\mathrm{CO}(\mathrm{g})+{\mathrm{H}}_2\mathrm{O}(\mathrm{g})\rightleftharpoons {\mathrm{CO}}_2(\mathrm{g})+{\mathrm{H}}_2(\mathrm{g})$ PAEV 1 2 3 4 NEXT Based on your ICE table (Part 2), set up the equilibrium expression for $\mathrm{Kc}$ in order to determine concentrations of all species. Each reaction participant must be represented by one tile. Do not combine terms. $K_c==5.1$