Question

19. Compound A decomposes to B and C according to the following equation: 2A(g) > B(g) + 2 (g) At 100 Celcius, 1.45 mol of A were placed in a 5.00 L container, and the reaction was allowed to proceed. After equilibrium was established, it was found that 67.9% of A had decomposed. What is the value of Kc for this reaction at 100 Celcius? a. 0.371 b. 0.343 c. 0.441 d. 0.407 e. 0.609

Answer 1

Big) +ac 2A(g) initial mol J 1.45 mol concentratima mol volume (4) 1145 mol - 0.29 M 5.00L At epuilibrium 67.90 A has de composed that means 0.29 X 6769 = 0.197M 1000 f Amount A left = 0:29- 0.197 = 0.093M Preparing Ice Table fore it Z = initial c= change equilibrium E-

equilibrium constant kc is defined as the ratio of Product raised to power its stoichiometric to ratio of reachant raised to power its stoichiometric conc. of conc g k= [6] [c]² [A?

2A (9) B1g) + ac) initial 0.29 0 2x x change -2x 2 2x equilibrium 0.29-22 0.29-2X = 0.093 At equilibjum + 2x = +0.197 0.0985 so [B]=0.0185M [c]= 0.197 m CA] = 0.093 &= [B] [B]² [A]² (0.0985) (0.197) . = 0.447 (0.093)? so oprimc correct Answer