Decomposition of ammonium hydrogen sulphide, NH4HS, on heating in a sealed flask is an endothermic process.

NH4HS (s) ⇌ H2S (g) + NH3 (g) 

If Kp for this reaction is 0.11 at 25 ̊ C, determine the partial pressure of NH3 and the total pressure in the flask (atm) at equilibrium. Based on the Kp value, calculate the Kc for this reaction at the same temperature. Using Le Chatelier’s principle, explain how increasing the temperature would affect the equilibrium. What will happen to the pressure of NH3 if some H2S is removed from the flask 

(a) Calculate the Kc for the reaction 

(b) If an additional 0.03 mol of I2 was injected into the system, predict the direction of equilibrium shift. 

Sulphuryl chloride, SO2Cl2, gas dissociates reversibly into sulphur dioxide gas, SO2, and chlorine gas, Cl2. The reaction is endothermic. Suggest all the possible ways to increase the chlorine production. An amount of 0.20 mol of SO2Cl2 was placed into a 2-L vessel and allowed to reach equilibrium. Calculate the equilibrium constant for the reaction if the final concentration of Cl2 is 0.08 M. The system in equilibrium is disturbed by adding 0.14 mol of SO2Cl2 at the same temperature. Calculate the concentrations of sulphuryl chloride and chlorine at the new equilibrium. 

Nitrogen (IV) dioxide dimerised as follows,

                       2NO2(g) ⇌   N2O4(g)                   DH = -58.84 kJ

Sketch a graph showing how the concentrations of the reactant and product of the above reaction vary during the course of the reaction. At 100oC, the value of Kc is 5.0. Calculate Kp for the above reaction. Explain how the product  could be increased. If initially 1 mole of NO2 is filled into a 1 L vessel, determine the concentration of N2O4 at equilibrium.