A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 3.71 x 10-8 s-1 at 25°C. What is the half-life for the degradation of DDT in this experiment, in years? (1 year = 365 days)   Round your answer to 2 decimal places.

The rate constant for the reaction                         CH2=CH2(g) + H2(g)  →  CH3−CH3(g) was found to be 5.6x10−5 s−1 at 100oC and 2.8x10−4 s−1 at 121.7oC. What is the activation energy (in kJ/mol)?

A student obtained the following data for the decomposition of hydrogen iodide on a gold surface at 150 °C. HI(g) H₂(g) + ½/2 1₂(g) [HI], M seconds 9.23x10-2 0 4.62x10-2 521 2.31x10-2 781 (1) What is the half-life for the reaction starting at t=0 s? 1.16x10-2 (3) Based on these data, what is the rate constant for the reaction? 911 What is the half-life for the reaction starting at t=521 s? Does the half-life increase, decrease or remain constant as the reaction proceeds? (2) Is the reaction zero, first, or second order? Ms-1

Consider the hypothetical reaction A +B+ 2C → 2D + 3E where the rate law is ΔΙΑ = k[A][B]? At Rate An experiment is carried out where [A]o = 1.0 x 10-² M, [B]o 6.0 M, 2 and [C, = 2.0 M. The reaction is started, and after 5.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. -2 k = L² mol -1 S b. Calculate the half-life for this experiment. Half-life = c. Calculate the concentration of A after 19.0 seconds. Concentration M d. Calculate the concentration of C after 19 seconds. Concentration = M

The generic reaction     2 A   →   products     follows zero-order kinetics with a rate constant of 0.00628 M/s.  What is the half-life of substance A if its original concentration is 2.23 M? Be sure to enter a unit with the answer.

The gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g) → 2 NO,(g)+% 02(g) is first order in N,Og. During one experiment it was found that when the initial concentration of N,0, was 8.25x10 M, the concentration of N,Os dropped to 1.42x10 M after 251.0 s had passed. Based on this experiment, the rate constant for the reaction is

Consider the following reaction. aA +bB →→ cC whose first and second half-lives are 18.4 and 36.8 minutes respectively.  If the rate constant is equal to 0.005408 and [A]0 = 10.05,  calculate the [A] at t = 23.12 minutes.

The rate law for the reaction 2NO(g) + 2H₂(g) N₂(g) + 2H₂O(g) is rate = K[NO]²[H₂] -1 If the rate of reaction is 4.66 × 10-3 mol L-¹s¹ when the concentrations of NO and H₂ are both 6.9 x 10-6 mol L-¹, what is the value of the rate constant and what are the units for the rate constant? k= i x 1013 X 9.56 5-1 mol L-¹5-1 L³ mol-³ s-1 3 L² mol-2 s-1 L mol-¹ S-1

The OH radical reacts with itself in a disproportionation type reaction according to the reaction: OH  +  OH  →  H2O  +  O  This rate constant at room temperature is 2.69 x 102 M-1 s-1. If the initial concentration of OH is 2.60 x 10-5 M, what is the first half life for the reaction (in seconds)?

The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows. C12H22011 + H20 → C;H1206 + CgH1206 This reaction follows a first-order rate equation for the disappearance of sucrose: rate = k [C,,H,,0,1] (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, i.e. they are 22 isomers.) 1.8x10-11 Arrhenius equation at this temperature). (Enter unrounded values.) (a) In neutral solution, k at 26°C and 8.5x10-11 -1 at 37°C. Determine the activation energy (in kJ/mol), the frequency factor (in s), and the rate constant (in s) for this equation at 48°C (assuming the kinetics remain consistent with the activation energy 108 kJ/mol frequency factor rate constant X s-1 (b) When a solution of sucrose with an initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40x10 M. How long (in s) will it take the solution to reach equilibrium…