In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g H2(g) + % I(g) the following data were obtained: (HI], M 0.401 0.201 0.101 5.05-10 seconds 519 779 910 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.401 M is and when the starting concentration is 0.201 M is (2) The average rate of disappearance of HI from t=0s to t= 519 s is (3) The average rate of disappearance of HI from t= 519 s to t= 779 s i Ms! (4) Based on these data, the rate constant for this v order reaction is Submit Answer Retry Entire Group 9more group attempts remaining

The first order rate constant for the decomposition of a certain hormone in water at 25 degrees C is 3.42 x 10-4 day-1.  a)If a 0.0200 M solution of the hormone is stored at 25 degrees C for 2 months, what will its concentration be at the end of that period? b)How long will it take for the ocncentration of the oslution to drop from 0.0200 M to 0.00350 M? c)What is the half-life of the hormone?

The decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C N,052 NO, + ½ O2 is first order in N,05 with a rate constant of 4.10x103 min!. If the initial concentration of N,O3 is 0.348 M, the concentration of N,Og will be 8.63×102 M after| have passed. min

Using the information provided, determine the activation energy for the reaction. Please explain why the hilighted answer is correct.. thank you!

In a study of the decomposition of ammonia on a tungsten surface at 1100 °C NH31/2 N2 + 3/2 H, the following data were obtained: NH3), M seconds 7.30x10-3 440 1.46x10-2 3.65x103 1.83×10-3 660 770 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 1.46x1o-² M i starting concentration is 7.30×103 M is| s and when the (2) The average rate of disappearance of NH3 from t= 0 s to t= 440 s is Ms. (3) The average rate of disappearance of NH3 from t= 440 s to t= 660 s is |Ms. (4) Based on these data, the rate constant for this| order reaction is Ms!.

The Nobel Prize in Chemistry was awarded in 1995 to Paul Crutzen, Mario Molina and Sherwood Rowland for research showing the chlorofluorcarbons (CFCs) were catalyzing the destruction of ozone in the stratosphere.  The catalytic process can be described by a two step mechanism: (1) Cl + O3 --> ClO + O2   (slow) (2)  ClO + O --> Cl + O2 (fast) Determine the overall reaction for this mechanism, and answer the following question: In this mechanism Cl acts as a(n) ______________  and ClO acts as a(n) ___________________.   a. reagent, intermediate   b. intermediate, catalyst   c. catalyst, intermediate   d. intermediate, product

The frequency factor and activation energy for a chemical reaction are A = 5.48 x 10-12 cm/(molecule-s) and E, = 15.6 kJ/mol at 382.7 K, respectively. Determine the rate constant for this reaction at 382.7 K. cm/(molecule•s)

In a study of the decomposition of nitrous oxide at 565 °CN2O(g)N2(g) + ½ O2(g)the following data were obtained: [N2O], M 2.10 1.05 0.525 0.263 seconds 0 602 1.81×103 4.21×103 Hint: It is not necessary to graph these data.(1)The observed half life for this reaction when the starting concentration is 2.10 M is s and when the starting concentration is 1.05 M is s.(2)The average (1/[N2O]) / t from t = 0 s to t = 602 s is M-1 s-1.The average (1/[N2O]) / t from t = 602 s to t = 1.81×103 s is M-1 s-1.(3)Based on these data, the rate constant for this  order reaction is M-1 s-1.

Pls show all steps with explanation

[4] The reaction: 21 (aq) + S2O;²-(aq) → I½(aq) + 2SO,²-(aq) is first order with respect to I and first order with respect to S20g. The rate constant k was determined at different temperatures and a plot of In(k) versus 1/T was constructed resulting in the straight line: y = -5781.8x + 14.1. Assume k has units of M's. (a) Determine the activation energy for this reaction. (b) Calculate the value of k at 20 °C.