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A mixture containing 19.8 moles of H2 and 7.2 mole of I2 was allowed to reach equilibrium in a 5 L closed vessel at ToC according to the equation: H2 (g) + I2 (g) 2HI (g) At equilibrium, 14 moles of H2 was present. The equilibrium constant for this reaction is denoted as Kc(1).
(a) How many grams of hydrogen iodide (HI) will be produced if a mixture of 45 g I2 and 0.5 g H2 was allowed to reach equilibrium in a 100 L closed vessel at T oC? (2 marks)
(b) If chlorine (Cl2) gas is added to the above reaction system, a new equilibrium will be established with an equilibrium constant denoted as Kc(2).
2HI (g) + Cl2 (g) ↔ 2HCl (g) + I2 (g)
(i) Express the equilibrium constant Kc(2) in term of Kc(1). (1 mark)
(ii) An unknown amount of Cl2 gas is added to the system in Question 3(a). so that there is 40.0 g Cl2 at equilibrium. Calculate the number of moles of hydrogen chloride (HCl) gas produced if Kc(2) is twice than that of Kc(1). (2 marks)
(iii) What will be the position of equilibrium for the overall reaction if more HI is added to the reaction mixture at constant temperature and pressure? Explain your answers.
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