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 rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH,NCO(aq)→(NH2)½CO(aq) the concentration of NH,NCO was followed as a function of time. It was found that a graph of 1/[NH,NCO] versus time in minutes gave a straight line with a slope of 1.45×10² M' min and a y-intercept of 1.67 M!. Based on this plot, the reaction is| | order in NH,NCO and the rate constant м1 min1 for the reaction is

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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 =

In a study of the conversion of methyl isonitrile to acetonitrile in the gas phase at 250 °CCH3NC(g)CH3CN(g)the concentration of CH3NC was followed as a function of time.It was found that a graph of ln[CH3NC] versus time in seconds gave a straight line with a slope of -4.38×10-3 s-1 and a y-intercept of -2.83 . Based on this plot, the reaction is ______ order in CH3NC and the half life for the reaction is _______ seconds.

The decomposition of hydrogen peroxide in the presence of potassium iodide is believed to occur by the following mechanism: step 1: H2O2 +I H20 + OI step 2: H2O2 + OI –H20 + O2 +I (a) Identify the molecularity of each step in the mechanism. step 1 step 2 (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (c) Identify any intemediates in this mechanism. Intermediate: Enter formula. If none, leave box blank:

Calculate the velocity of the reaction (M · s–1) of an α-amino group in a blood protein at 37°C if its concentration is 0.60 mM and the partial pressure of carbon dioxide is 40 torr. Use 2 significant figures and scientific notation (example: 1000 would be entered as 1.0e+3). The rate constant k for this reaction is 4950 M–1·s–1.

How do you calculate the concentrations using the absorbance?

The first-order rate constant, k1, for the decomposition of ampicillin at pH 5.8 and 35?C is k1 = 2 × 10-7 sec-1. The solubility of ampicillin is 1.1 g/100 mL. If it is desired to prepare a suspension of the drug containing 2.5 g/100 mL, calculate the zero-order rate constant, k0, and the shelf-life, that is, the time in days required for the drug to decompose to 90% of its original concentration (at 35?C) in solution. Note: 100 mL = 1 deciliter = 1 dL.

-1000 Decomposition Rezctions Carbon Reduction Reactions AH AS (kJ) (JK-mol) O 2 Ag,0(s) → 4 Ag(s) + O2(g) +62.2 +132.7 O 2 MgO(s) → 2 Mg(s) + O2(g) +1202.4 +216.7 1000- O 2 AlhO3(s) → 4 Al(s) – 3 02(g) +3351.4 +546.8 O 2 Fe2O3(s) → 4 Fe(s) – 3 O2(g) +1648 4 +5515 O 2 HgO(s) → 2 Hg(t) + 0,(g) +181.7 +286.8 2000- O 2 Cr,03(s) → 4 Cr(s)– 3 0,(g) 2269 4 +548.4 Temperature 3000 300 300 K 2000 Temperature ((K) Clear Graph The metals Mg and Al, like most metals in groups 1A, 2A, and 3A of the periodic table, cannot be obtained by chemical reduction with carbon at reasonable temperatures. What procesS Is used to obtain these metals from their ores? positive