Consider the following reaction for which K 1.60 x 10 at some temperature 2 NOCl (g) ㄹ 2 NO (g) + Cl2(g) In a given experiment, 0.935 moles of NOCI(g) were placed in an otherwise empty 1.51 L vessel. Complete the following table by entering numerical values in the Initial row and values containing the variable “x” in the Change and Equilibrium rows. Define 2x as the amount (mol/L) of NOCI that reacts to reach equilbrium. Include signs in the Change column to indicate a gain or loss of concentretion. (Omit units, use 3 sig·fig. and write concentrations less than 1 as o.###, not as .###. If nothing is present initially, enter 0 for the molarity.) INOCI] (M) [NO] (M) Initial Change Equilibrium Submit Answer Tries 0/10 Since K is very small, K 1.60 x 10-7, very little product will be present at equilibrium, which tells us that very little NOCI will react to reach equilibrium. Because of this, the equilibrium concentration of NOCI will remain, essentially, at its initial concentration. Making this assumption, calculate the equilibrium concentration of NO. Note: use the ICE table from the previous problem to help you solve this problem. (Scientific notation can be entered using the following convention: 1.93x 101.93E-3.) NOlea Submit Answer Tries 0/99