Use these three elementary reactions: \text { Rxn 1: } \mathrm{C}_{2} \mathrm{H}_{2}+2 \mathrm{Cl}_{2} \rightarrow \mathrm{C}_{2} \mathrm{H}_{2} \mathrm{Cl}_{4} \operatorname{Rxn} 2: 3 \mathrm{H}_{2}+\mathrm{N}_{2} \rightleftharpoons 2 \mathrm{NH}_{3} \mathrm{Rxn} 3: 2 \mathrm{~F}_{2}+\mathrm{CH}_{4} \rightarrow 2

\mathrm{H}_{2}+\mathrm{CF}_{4} For each case, if the feed is stoichiometric, say so, if not, identify the Limiting Reactant i Rxn 1, feed is 50% C2H/50% Cl2 ii. Rxn 2, feed is 25% N/75% H2 iii. Rxn 3: feed is 35% CH/60% F/5% H2 b. Show the Stoichiometric Table for each reaction. c. Write the rate law for each reaction and indicate the proper units (using s (for time),mol/l (for conc.), atm (for partial pressure), and g for cat. wt.) for each rate constant,as well as for the equilibrium constant for reversible reactions. i Rxn 1, using concentrations ii. Rxn 2, using partial pressures... ili. Rxn 3, catalytie reaction using concentrations d. Now assume the value of the rate constant in terms of the Limiting Reactant is 1.4 (withthe appropriate units) and calculate the rate constant for each of the other species(including the products) in each reaction.