Urea (NH2CONH2) is the end product in protein metabolism in animals. The decomposition of urea in 0.1 M HCl occurs according to the reaction NH2CONH2(aq)+H+(aq)+2H2O(l)→2NH4+(aq)+HCO3- (aq) The reaction is first order in urea and first order overall. When [NH2CONH2]= 0.200 M, the rate at 61.05 ∘C is 8.56×10-5 M/s. What is the value for the rate constant, k?

The formation of iodine is described by the following chemical equation: H, (g) + 2IC1 (g) → 2HC1 (g) +Iz (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: H, (g) + IC1 (g) НI (g) + HCI (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.

The gas phase decomposition of dinitrogen pentoxide at 335 K 2 N205 →4 NO2+02 has the following relationship between rate and concentration, where the bracket around the formula indicates concentration and k is a constant called the rate constant. Rate = k[N2O5l %3D If the value of k is 7.38×10~$ s', what is the rate of the reaction when [N2O5] = 0.180 M? Ms-

For the reaction: 3 Ag  +  NO3–  +  4 H+  –––>  NO  +  2 H2O  +  3 Ag+ If the rate of disappearance of Ag is 0.0017 mol L–1 s–1, what is the rate of the appearance of water? For the 1st order reaction:   A ––> products,    assume the concentration of A falls to one-third of its original value after 150 seconds.  Calculate the rate constant and the half-life.

The decomposition of nitramide in aqueous solution at 25 °C NH2NO2(aq)–N20(g) + H20(1) is first order in NH,NO2 with a rate constant of 0.0000470 s1. If the initial concentration of NH2NO2 is 0.548 M, the concentration of NH2NO2 will be 0.0986 M after s have passed.

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Suppose the reaction between nitric oxide and oxygen proceeds by the following mechanism: step elementary reaction rate constant 1 NO(g) + O,(g) –→ NO2(g) + O(g) k1 NO(g) + O(g) → NO2(g) Suppose also k,«k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k || Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k-2 for k = | %3D the reverse of the two elementary reactions in the mechanism.