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12 Nov 2019
6. (1 pts) (a) Show by calculation if the following gas phase reaction is at equilibrium, with the molar concentration conditions stated under each participant. (Hint: Q reaction quotient). For this temperature, K = 1.45 x 104 Instantaneous concentrations, M: 5.4x 104 9.7x 10-3 4.5 x 10- 2.3 x 10 (b) (0.5 pt) Based on your calculation in part (a) what will be observed over time, in the reaction vessel? Circle one: more NO will fornm more NH3 will form no change 7. (a) (0.9 pts) The balanced equation for the acid dissociation of acetic acid is given below. Make an "ICE" table showing the initial concentrations, change in concentration and equilibrium concentrations of the three clh in the reaction. Initial concentration of the acetic acid is 0.0575 M Initial: Change: Equilibrium Ka, acetic acd1.75 x 10 CHyCOO-(aq) H+ (aq) ã¹ + CH3COOH (aq) (b) (0.6 pt) Use the data in the "ICE" table and the K, stated in the problem to calculate the equilibrium value of [H+. H+1
6. (1 pts) (a) Show by calculation if the following gas phase reaction is at equilibrium, with the molar concentration conditions stated under each participant. (Hint: Q reaction quotient). For this temperature, K = 1.45 x 104 Instantaneous concentrations, M: 5.4x 104 9.7x 10-3 4.5 x 10- 2.3 x 10 (b) (0.5 pt) Based on your calculation in part (a) what will be observed over time, in the reaction vessel? Circle one: more NO will fornm more NH3 will form no change 7. (a) (0.9 pts) The balanced equation for the acid dissociation of acetic acid is given below. Make an "ICE" table showing the initial concentrations, change in concentration and equilibrium concentrations of the three clh in the reaction. Initial concentration of the acetic acid is 0.0575 M Initial: Change: Equilibrium Ka, acetic acd1.75 x 10 CHyCOO-(aq) H+ (aq) ã¹ + CH3COOH (aq) (b) (0.6 pt) Use the data in the "ICE" table and the K, stated in the problem to calculate the equilibrium value of [H+. H+1
Jamar FerryLv2
26 Sep 2019