In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH,NCO(aq)+(NH2)2CO(aq) the concentration of NH4NCO was followed as a function of time. It was found that a graph of 1/[NH₂NCO] versus time in minutes gave a straight line with a slope of 1.74x10-2 M-1 min¹ and a y-intercept of 2.34 M-¹. Based on this plot, the reaction is M1 min¹. ✓order in NH4NCO and the rate constant for the reaction is

The enzyme carbonic anhydrase catalyzes the reactionCO2(g) + H2O(l)--->HCO3- (aq) + H+(aq). In water,without the enzyme, the reaction proceeds with a rateconstant of 0.039 s-1 at 25 °C. In the presence of the enzymein water, the reaction proceeds with a rate constantof 1.0 x 106 s-1 at 25 °C. Assuming the collision factor isthe same for both situations, calculate the difference inactivation energies for the uncatalyzed versus enzymecatalyzedreaction.

(4a) The following initial rate data are for the reduction of nitric oxide with hydrogen:2 NO + 2 H2N2 + 2 H2O Experiment [NO]o, M [H2]o, M Initial Rate, M s-1 1 0.438 0.289 7.93×10-2 2 0.876 0.289 0.317 3 0.438 0.578 0.159 4 0.876 0.578 0.634 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate =     From these data, the rate constant is ____________ M-2s-1. (4b) The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution:NH4+ + NO2- N2 + 2 H2O Experiment [NH4+]o, M [NO2-]o, M Initial Rate, Ms-1 1 0.710 0.152 3.38×10-5 2 0.710 0.303 6.73×10-5 3 1.42 0.152 6.76×10-5 4 1.42 0.303 1.35×10-4 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not…

The rate of the elementary reaction O2 + H2H + HO2 has been studied as a function of temperature between 1000 and 1400 K. The following data were obtained for the rate constant k: (a) Calculate the activation energy of this reaction. kJ mol-1 (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant.