In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH,NCO(aq)(NH2)½CO(aq) the concentration of NH4NCO was followed as a function of time. It was found that a graph of 1/[NH4NCO] versus time in minutes gave a straight line with a slope of 1.44×102 M- min-1 and a y-intercept of 0.980 M-1. | order in NH4NCO and the rate constant for the Based on this plot, the reaction is | M' min-!. reaction is

In a study of the gas phase decomposition of nitrogen dioxide at 383 °C NO₂(g) →→→NO(g) + ½ O₂(g) the concentration of NO₂ was followed as a function of time. It was found that a graph of 1/[NO₂] versus time in seconds gave a straight line with a slope of 0.815 M-¹ s¹ and a y-intercept of 11.5 M-¹. Based on this plot, the reaction is [ ✓order in NO₂ and the rate constant for the reaction is M-¹ S-¹.

In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH,NCO(aq)–→{NH2)½CO(aq) the following data were obtained: [ΝHNCO], M 1.14 0.570 0.143 0.285 minutes 95.6 287 667 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.14 M is min and when the starting concentration is 0.570 M is min. (2) The average A(1/[NH,NCO]) / At from t= 0 min to t = 95.6 min is M min-! The average A(1/[NH¼NCO]) / At from t = 95.6 min to t = 287 min is м1 min1. (3) Based on these data, the rate constant for this order reaction is M min!.

In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)- → H₂(g) + ½ I₂(g) the concentration of HI was followed as a function of time. It was found that a graph of 1/[HI] versus time in seconds gave a straight line with a slope of 1.64×10-³ M-¹ s-¹ and a y-intercept of 0.418 M-¹. Based on this plot, the reaction is order in HI and the rate constant for the reaction is M-¹ S-¹.

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In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH,NCO(aq)→(NH2)½CO(aq) the following data were obtained: [NH,NCO], M |0.715 8.95x10-2 1.05x103 0.358 0.179 minutes 150 449 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.715 M is min and when the starting concentration is 0.358 M is min. (2) The average A(1/[NHẠNCO]) / At from t= 0 min to t= 150 min i | The average A(1/[NH,NCO]) / At from t= 150 min to t= 449 min is M min. M' min!. (3) Based on these data, the rate constant for this | order reaction is M' min!.

In a study of the decomposition of nitrous oxide at 565 °CN2O(g)N2(g) + ½ O2(g)the concentration of N2O was followed as a function of time.It was found that a graph of 1/[N2O] versus time in seconds gave a straight line with a slope of 1.55×10-3 M-1 s-1 and a y-intercept of 0.952 M-1.Based on this plot, the reaction is     order in N2O and the rate constant for the reaction is M-1 s-1.

In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of [HI] versus time in seconds gave a straight line with a slope of -1.91×10-4 Ms and a y-intercept of 0.235 M. Based on this plot, the reaction is reaction is order in HI and the rate constant for the Ms!

In a study of the decomposition of nitrous oxide at 565 °C N₂O(g) N₂(g) + ½ O₂(g) the concentration of N₂O was followed as a function of time. It was found that a graph of 1/[N₂O] versus time in seconds gave a straight line with a slope of 1.63×10-³ M-¹ S-¹ and a y-intercept of 0.463 M-¹. Based on this plot, the reaction is M-¹ S-¹. order in N₂0 and the rate constant for the reaction is

The decomposition of hydrogen peroxide in the presence of potassium iodide is believed to occur by the following mechanism: step 1 slow: H2O2 +I→H20 + OI step 2 fast: H202 + OI → H20 + 02 +I (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]"B]".. , where '1' is understood (so don't write it) for m, n etc.) Rate =