The reaction A -> B is first order with a half life of 0.854 seconds. What is the rate constant of this reaction in s-1? Answer with 3 places past decimal point

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The reaction A-B is first order with a half life of 0.903 seconds. What is the rate constant of this reaction ins 1? Do not report units in your answer. Report your answer with 3 places past the decimal point. Type your answer..

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Q5 - Half-life Homework • Unanswered lodine atoms combine to form molecular iodine in the gas phase. This second order reaction has a rate constant of 7.0 x 109 1/(M*s). Calculate the time required for the iodine concentration to decrease from 0.60 M (t=0) to 0.30 M. Note: this specific time is known as the half-life of the reaction. |(g) + I(g) → I2(g) -> |2{8) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a 2.4 x 10-10 s b 9.9 x 10-11 s 4.3 x 10-11 s

rate = k [A]1 [B]1  (k = 5.8 M-1∙s-1) Using the above rate law, deduce what volumes of the A and B solutions, and water would need to be combined to achieve a color change at the 90 second mark (you can disregard the need for the B-dilution solution).  You must annotate your calculations (tell me why you are doing what you are doing).  Remember that the total volume will need to be 20 mL, and that the starting concentrations of the A is 0.0090 M,  and B is 0.0050 M.

The reaction A→ Products is a first-order reaction with a rate constant of 1.91 x 10-3 min-1. The reaction started with an initial concentration of A equal to 0.0881 M, what is the concentration of A after 131.1 minutes? Do not write unit in answer. Report your answer with four places past the decimal point. Type your answer... Submit