Please help with question 5. Please ignore my work as it is wrong and needs correcting! Thank you!

PU! ha 5) The reaction below has the following equilibrium constant 2 H20 (1) = H20+ (aq) + OH- (aq) comat is not required K = 1.00 x 10-14 0.ODODDOOOOOO! The concentrations in a reaction that is in progress are [H30*1 = 0.0023 M and (OH) = 0.0052 M. Calculate Q, compare with K and determine in which direction the reaction proceeds. So a must incrouse in order to reach 3 due to a being smaller than K. Q=12420] /[H0* senza 10023, 123 10052 6) The reaction shown in question 5 has reached equilibrium. Now, you add some hydroxide ions. Using a) a kinetic argument, b) change in Q and c) Le Chtelier's principle, predict whether the reaction is still at equilibrium, will proceed in the forward direction or will proceed in the backward direction. a. Kinetic argument (changes in the forward and backward reaction rates) Correct Adding Tite but Rewing product slows the reverse ree does not immedietly of feat the reaction rate. (-7 hat Forwirs) Removing product will enable b. How Q changed relative to K 12 to be smalles. This is that with c. Using Le Chtelier's principle 1 can A alk, reartion States that removing the product will result in the reaction making more product, When the 01 rea