Question

12. If the acetic acid dissociation constant is 1.8 X 10-5 Ka, and its concentration before dissociation (0.15M), the concentration of H+] is equal to the following equilibrium equation. CH,COOH = CH.COO+H* B) 6.41 X 104 C)2.62 X 104 D)1.64 X 10 13. When dissolved (1.93 g) of HNO, acid (MW=47) and dilute the volume to 500 ml the H concentration in the solution was 7.63X10 M, the value of the dissociation constant Ka was equal to : A) 8 X 104 B) 6 X 104 C) 4 X104 D) 2 X 104 14. Hydrogen iodide disintegrates at (458°C) according to the following equation 2HI(g) + H:(8) +12(g) If (4 mol) of (HI) is placed in a container of (SL) at (458 ° C) and found that the container contains (0.442 mol) of (12), the equilibrium constant is equal to: B) 0.052 A) 0.021 C) 0.092 D) 0.010 effect of increased pressure on the system in the following 15. Determine the effect of increased pressu equilibrium CO(g) + Cl2 + COCL2 (g) A) The equilibrium position SHIFT to the right B) The equilibrium position SHIFT to the lo s not change the position of equilibrium bes not apply to the system C) does not change the position D) The Le Chatelet principle does not app

Answer 1

CH] = ( kaxc = {(1,5x108) (0.15) = 1.64x16 -3 Answer: D 1-64 x 10 ® JEC- 47 HNO3) = c = 1-93 x t = 0.0821 3 mots ka = [H+] = 7.63x103) C-[ht] 0,0821-(7.63X16 = 7.8* To 4 6. = *Xia Answer: A sxTot (6.402 4 Kc = I LIL). [H2] [I] = 1 CHIJ2 (4-0.4 = 0.010 answer: D 01010 6 Answer: ④ Aญเง4: