(a) The reversible reaction of compound X with compound Y can be expressed in terms of an elementary forward second-order reaction (with rate constant, ki) and an elementary reverse first-order reaction (with rate constant, kr), X+Y AZ k, Based on this expression, develop an equation relating the equilibrium constant K= 106.8 for this reaction to the rate constants ky and kr. Now, if kr 104 s-?, use this equation to estimate the value of ks (inclusive of the correct units). (b) The following represents experimental data collected by measuring the disappearance of a compound, A, (with concentration in mg/L) versus time. 0.06 0.05 0.04 0.03 0.02 0.01 1/A = 0.012 + (9.8 x 10-3) r2 = 0.974 1 1 1 1 1 2 3 4 t, hr 0.00 5 6 Is this a zero-order, first-order, or second-order reaction? Why? What is the rate constant for this reaction, reported with the correct units