Question 3. (a) In an aqueous solution of CH3NH3 the following equilibrium is established. CH3NH3 (aq) + H2O (1) CH3NH3* (aq) + OH° (aq) Determine Kc for this equilibrium at 298 K if the initial concentration of CH3NH3 is 0.1 M and at equilibrium the concentration of OH is 0.0066 M.

Enter your answer in the provided box. Consider the following reaction at a high temperature. Br2(g) 2Br(g) When 1.30 moles of Br2 are put in a 0.710-L flask, 1.90 percent of the Br2 undergoes dissociation. Calculate the equilibrium constant Ke for the reaction.

Suppose the following reaction is at equilibrium: PCl3 + Cl2 ⇋ PCl5. (a) Are the equilibrium concentrations of PCl3, Cl2, and PCl5 necessarily equal? Explain. (b) Is the equilibrium concentration of PCl3 necessarily equal to that of Cl2? Explain.

Consider the following reversible reaction at equilibrium: C6H12O6(aq) + 6 O2(g)      6 CO2(g) + 6 H2O(l). Given that this reaction is exothermic, if heat is added to the equilibrium system, how is the stress relieved?

The following reactions all have K > 1. 1) CH3COO (aq) + C,H;COOH (aq) =CH;C0OH (aq) + CgH;C00 (aq) 2) CN (aq) + CgH;COOH (aq)= C,H3C00 (aq) + HCN (aq) 3) CH;COОH (аq) + CN (aq) — НCN (aq) + CH;COО (аq) Arrange the substances based on their relative base strength. Clear All C,H;COOH C,H;C00- strongest base CN- intermediate base CH3CO0 weakest base HCN not a Bronsted-Lowry base CH;COOH

Calculate K'p for the following reaction: 3CH3OH(g) 3CO(g) + 6H2(g)

Consider the reaction below at a certain temperature and pressure.The reaction begins with only [CO2] of 0.200 M and the equilibrium constant (Kc) is 9.81 X 10-6, what is the equilibrium concentration of H+ and HCO3-?

Acetaldehyde (CH3CHO) is an important chemical both industrially and biologically.  For instance, it is a (somewhat toxic) intermediate in the body's metabolism of ethanol into acetic acid, and thus is possibly implicated in the "hungover" symptoms of someone who has had too much to drink the night before.  In aqueous solution, it establishes an equilibrium with a hydrated form, shown below. CH3CHO (aq)   +   H2O (l)   <-->  CH3CH(OH)2 (aq) You start with an aqueous sample, already at equilibrium, with the CH3CH(OH)2 (the hydrated form) at a concentration of 2.60 M.  You have no information about how much, if any, of the anhydrous form (CH3CHO) is initially in the flask.  If you add 2.0 M of CH3CHO to the reaction flask, and as the equilibrium is being restored the amount of CH3CH(OH)2 changes by 1.13 M, what is the final amount of CH3CHO?

2. Calculate Q and compare it to K for the following conditions to indicate if the reaction proceeds forward or in reverse. CH;COOH (ag) + NO2"(aa) CH3CO0' (ag) + HNO2 (a9) K=0.045 a. [CH;COOH] = 0.010 M, [NO2] = 0.10 M, [CH;COO']= 1.0 M, [HNO2] = 0.50 M b. [CH;COOH] = 0.102 M, [NO2"] = 0.10 M, [CH;COO']= 0.021 M, [HNO2] = 0.019 M

Consider the following equilibrium for which H = -114.44: 4 HCl(g) + O2(g)  2 Cl2(g) + 2 H2O(g) How will each of the following changes affect an equilibrium mixture of the 4 gases in this reaction?(a) O2(g)) is added to the system. which will happen? the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease   (b) The reaction mixture is cooled. the equilibrium will not shift the equilibrium will shift toward product but Keq will not change the equilibrium will shift toward reactant but Keq will not change the equilibrium will shift toward product and Keq will increase the equilibrium will shift toward reactant and Keq will decrease  (c) The volume of the reaction vessel is reduced by 50%.       (d) A catalyst is added to the reaction mixture.       (e)…