Can you help me to explain step by step with number 2? Can you explain it to me? ● Definition of equilibrium• Keq: law of mass action●Le Chatelier's PrincipleTopics:●●●Properties of acids & basesBrønstead-Lowry Acids & Bases definitionKw & calculating [H3O+], [OH-], pH1. If the reaction below is initially at equilibrium, and then each of the following changes are made, predictwhich direction the reaction rate will be fastest until equilibrium is once again established: forward,reverse, or no change.H2(g) + Cl2(g) 2 HCl(g)a. the concentration of H₂ is increased forwardb. the concentration of HCl is decreased forwardc. the concentration of Cl₂ is decreased versc2. If the reaction below is initially at equilibrium, and then more NH4* is added, predict which direction thereaction rate will be fastest until equilibrium is once again established: forward, reverse, or nochange. ForwardIf more Hu is addedIf more wHyt addel, forwa rol NH4* (aq) + H₂O (1) NH3 (aq) +Hut reactantreaction fast until equilibriumreestablished-1[30+ (aq)3. Define (a) reversible reaction and (b) equilibrium.A) Reversible reaction isproduce original reactant,one where the products of the reaction can themselves react toB.) Equilibrium: Amount of reactant reach a balance istay there,4. For the reaction below: reverse reaction take place exactly same rate in both directionReaction takes place in both direction but over all effect forward's2 NO2 (g) + O2 (g) 2 NO3 (g)a. Write the law of mass action (the equilibrium expression for Keq)Keq = [03]кед[c]c[d] ProductsAja (B]b reactants[0₂] [NO₂]²b. If gas concentrations are as follows, 2.10 M NO2, 1.75 M O2, and 1.00 M NO3, calculate Keq1.00m]0.130x102(1.00m)0.1295Keq=(2.10m) ³x (675m) 0.130m²(4.41m x1.75m) 0.130c. Based on the Keq value that you calculated in part b, are the reactants or products predominant(predominant means that there is a greater amount present)?Keq is a less than 1, then equilibrium will shift toreverse direction. Change Made to a Reactionthat was at Equilibrium:Increase the concentration of a reactant.Increase the concentration of a product.Decrease the concentration of a reactant.Decrease the concentration of a product.Response:Rate of the forward reaction becomes greater than the rateof the reverse reaction until equilibrium is reestablished.Rate of the reverse reaction becomes greater than the rateof the forward reaction until equilibrium is reestablished.Rate of the forward reaction becomes less than the rate ofthe reverse reaction until equilibrium is reestablished.Rate of the reverse reaction becomes less than the rate ofthe forward reaction until equilibrium is reestablished.

Given eqm rxn: NH4+ ( aq) + H2O (l) <=> NH3 (aq) + H3O+ (aq) According to Le Chatelier…

2. If the reaction below is initially at equilibrium, and then more NH4* is added, predict which direction the reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no change. Forward If more If more wHyt added, forward NH4+ (aq) + H₂O (1) eaction fast until equilibrium Hui Hut reactant NH3 (aq) + H30* (aq) is added

2. If the reaction below is initially at equilibrium, and then more NH4* is added, predict which direction the reaction rate will be fastest until equilibrium is once again established: forward, reverse, or no change. Forward If more If more wHyt added, forward NH4+ (aq) + H₂O (1) eaction fast until equilibrium Hui Hut reactant NH3 (aq) + H30* (aq) is added

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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