Question

#1000K? 12. The equilibrium constant,ke, for the reaction H() + 12(g) 2 HI(g) 13542 0 40 mol sample of HI was introduced into a 1,00 mL reaction vessel at 125 °C, what are the equibrium concentrations of H2. 12, and HI? 13. Consider the following reaction which is at equilibrium at 25°C: 2NH3(g) + CO2(g), Alº - 152.2 kJ (c) the temperature is increased In which direction will the reaction shini (a) the pressure is increased (b) the pressure is decreased (d) the temperature is decreased? (e) some CO2 is added? () NH3 is removed? () a catalynt is added ? c) some NH (NH,CO2) is added? (1) some Ne is added? () the volume is increased? 14. Solid (NIT),S decomposes when heated as follows: (NH)S(8) = 2 NH3(g) + H2S(g) m) Write expresions for K, and show the relationship between them. b) What is if an equilibrium mixture was found to have pow of 0.50 atm c) What is for the reaction? 15. Write a balanced equation to show how you would make (NH4)2S. What is the name of this compound? 16. The equilibrium constant, K., for the reaction COCI(g) = CO(g) + Cl2(g) IN 8.4 x 10" at 360 "C. If an emty 50.0 L vessel is charged with a 1.00 mol of COCl2 at 360 °C, what is the total pressure in the container reaches equilibrium?

Answer 1

2HI(g 12) Equilibrium: H,(g)I(g) ; K 33 For reverse reaction 1 = 0.0303 33 2HI(g H2 (g) (g) ;K = 0.40 mol Concentrati on of HI 0.40 M 1.00 L The ICE table constructed is as follows 2HI(g) H2(g) (g) Initi al (M): 0.40 0 0 Change (M): -2x x Equilibrium (M): 0.40-2x H, Equilibrium constant, K HIP (x) (0.40-2x) 0.0303= 0.40 2x V0.0303 0.174 0.40 2x - 0.174(0.40-2x) x 0.0696- 0.348x 1.348x 0.0696 x 0.052 According to the ICE table, Equilibrium concentration of H [H] = (x) M 0.052 M Equilibrium concentration of I Equilibrium concentration of HI, [H] = (0.40-2x) M= (0.40-2x0.052) M = 0.052M = 0.296 M 0.30M