If the rate constant for this second-order reaction is 8.0 x 10^-8 L mol^-1 s -1 , what is the half-life for the decomposition of NOCL when the concentration of NOCL is 0.15 M?   8.0 x 10^8 s   1.24 x 10^8 s   0.15 s   8.3 x 10^7 s

Consider the reaction below. The reaction starts with an initial concentration [A] of 3.50x10-2 M and is tracked over time. The rate of change is then plotted versus time; the graph is initially nonlinear, but becomes linear when 1/[A] is plotted versus time. The slope of the graph was determined to be +1.80x10-2 L/mol s.aA → bB 1. Calculate the half life for this reaction.2. How much time (in seconds) is required for the concentration of A to decrease to 4.00x10-3 M?

Initial rates were measured for the following reaction and are listed in the table. A + 2B ⎯→ products   Expt. Initial Concentrations Initial Rate (mol/L·s) [A] [B] 1 0.115 0.135 2.70 × 10−3  2 0.115 0.270 2.16 × 10−2  3 0.345 0.135 8.10 × 10−3  What is the order of the reaction with respect to A, with respect to B, and overall?

A particular reactant decomposes with a half-life of 103 s when its initial concentration is 0.275 M. The same reactant decomposes with a half-life of 211 s when its initial concentration is 0.134 M. Determine the reaction order. 1 What is the value and units of the rate constant for this reaction? Units k = M-1.s-1 M·s-1 M-2.s-1

A chemistry graduate student is studying the rate of this reaction: 2H1 (g) - H₂ (g) +1₂ (g) She fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [HI] 1.00 M 0.227M 0.20 0.128M 0.30 0.0894M 0.40 0.0686M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate=& D.D

What is the activation energy of a reaction if it has the following rate constants?

In the presence of excess thiocyanate ion, SCN, the following reaction is first order in iron(III) ion, Fe+ The rate constant is 1.27/s. Fe+ (ag) + SCN(ag) → Fe(SCN)2+ (ag) If 35.7% of the reaction is required to obtain a noticeable color from the formation of the Fe(SCN)2+ ion, how many seconds are required? Time =

The rate constants for the decomposition of dinitrogen pentoxide are3.7x10-5 s-1 at 25 oC and 1.7x10-3 s-1 at 55 oC.2 N2O5 (g) → 4 NO2 (g) + O2 (g) -Determine the activation energy for this reaction in KJ/mol.

Your laboratory is asked to analyze a water sample for a particular pesticide. You know from previous study that this pesticide degrades via a first order, irreversible reaction. The first order rate constant (k) for the reaction at 4 °C is 0.02 day¹. The activation energy for the reaction is known to be 10 kcal/mol. The standard preservation method for water samples containing this pesticide is to store the sample at 4 °C for no more than 24 hours prior to analysis. Calculate the fraction of the pesticide that remains in the sample after 24 hours of storage at 4 °C. b. A newly hired staff member collects a sample of the water but forgets to store it at 4 °C. Instead, they leave the sample in the trunk of their car (average temperature 35 °C) over the weekend. 60 hours later the sample is analyzed and found to contain 0.01 mg/L of the pesticide. What was the pesticide concentration in the water at the time the sample was taken?