Anything that I've left unanswered please

a) An unknown compound decomposes according to the following reaction. The graphs below were A2B(g)A2(g)+B(s) time. The initial cone constructed with data pertaining to changes in [A2B] over concentration of A2B was of A2B was 0.045M. When 150 minutes passed the 1. wnat is the order of the overall reaction? Justify your answer. The order of the averall reaction is finst order. This is because the rater of the reaction ends up being proportional to the concentration of the reaurion. II. What is the rate law for the overall reaction? Rate=H[A] III. Calculate the rate constant, k, for the reaction? (Include units) A IV. What is the half-life for this decomposition? (Include units) k b) Draw approximations of the complete energy profile diagrams for the following catalyzed and uncatalyzed process. Label each curve. PCl5(g)PCl3(g)+Cl2(g)H=+87.9kJ c) A two step mechanism is outlined below. I2(g)2I(g)H2(g)+2I(g)2HI(g)(fastequilibrium)(slow) I. What is the overall reaction? II. Is I (g) a catalyst or an intermediate? Justify your answer. III. What is the rate law for the overall reaction? Justify your answer. 1. Write the balanced net ionic equation for the reaction. KI+FKF+I II. What is the oxidation number of fluorine before the reaction occurs? What is the oxidation number of fluorine after the reaction occurs? e) An acidified potassium dichromate solution is added to a solution of copper (I) chloride. I. Write the balanced net ionic equation for the reaction. II. What is the oxidation number on chromium in potassium dichromate? What is the oxidation number of chromium after the reaction occurs f) An acidified potassium permanganate solution is added to a solution of iron (II) sulfate. I. Write the balanced net ionic equation for the reaction. II. What is the oxidation number on manganese before the reaction? What is the oxidation number of manganese after the reaction occurs g) A solid piece of zinc is dropped into a gold (I) nitrate solution. I. Write the balanced net ionic equation for the reaction. II. Identify the species that was oxidized in this reaction