(Solved): For a reaction:2) The rate of the reaction A +3 B->C+ 2 D was reported as 2.0 mol dm-3s -1.3Al (s ...

For a reaction:2) The rate of the reaction A +3 B->C+ 2 D was reported as 2.0 mol dm-3s -1.3Al (s) + 202 (g) -> 2AbOs (s)A chemist observed that tripling and doubling the molar concentrationsaluminium and oxygen, respectively had no effect and doubled the initial rateof the products, respectively. Write down the rate order with respect to eachreactant and consequently the rate expression for this reaction.3) The rate of consumption of B in the reaction A + 3 B ->C+2 D is 2.0 mol dm-3s1. State the reaction rate, and the rates of formation or consumption of A, C,and D.State the rates of formation and consumption of the participants.A second-order reaction of the type A +2 B ->P was carried out in a solutionthat was initially 0.075 mol dm-3 in A and 0.030 mol dm-3 in B. After 2.0h theconcentration of A had fallen to 0.045 mol dm-35) A reaction 2 A ->P has a third-order rate law with k=3.50 x 10-4 dmmol-2 s-1.Calculate the time required for the concentration of A to change from 0.077 moldm-3 to 0.021 mol dm-3(a) Calculate the rate constant.6) The rate constant for the decomposition of a certain substance is 1.70 x 10*2dm mol1 s1 at 24\deg C and 2.01 x 10-2 dm mol1 s1 at 37\deg C. Evaluate theArrhenius paramneters of the reaction.(0)(b) What is the half-life of the reactants?7) At 400 K, the rate of decomposition of a gaseous compound initially at apressure of 12.6 kPa, was 9.71 Pas1 when 10.0 per cent had reacted and 7.67Pas- when 20.0 per cent had reacted. Determine the order of the reaction.(ü)8) At 400 K, the half-life for the decomposition of a sample of a gaseous compoundinitially at 55.5 kPa was 340 s. When the pressure was 28.9 kPa, the half-lifewas 178 s. Determine the order of the reaction.(üi)9) Derive the integrated rate law expression for a Zero order reaction involvingsingle reactant.10)Derive the integrated rate law expression for a second order reaction involvingtwo reacting species of unequal concentrations11) The data in the table were colected at 540K for the following reaction.CO(g) + NO2(g) -> COz(9) + NO(g)Reactant Concentration (mo/L)[CO]5.1 x 10-45.1 x 1045.1 x 10-41.0 x 1031.5 x 103|0.35 x 10-40.70 x 10-40.18 x 10-40.35 x 10-4|0.35 x 104[NO2]Calculate the rate constant for the reaction.Initial Rate(mol/L.h)3.4 x 10-86.8 x 10-81.7 x 10-86.8 x 10-8Find the expression for the rate law for this reaction.10.2 x 10-8Find the rate of appearance of CH3Cl at the instant when [CH3OH] =0.250M and [HCIJ=0.321 M