The rate constant for the first order reaction A ---> B + C is k = 0.016 min-1 at 300 K. What is the half-life for this reaction at 300 K?

The reaction A → B + C is zero order with respect to A. When [A]0 = 0.858 M, the reaction is 23.4 % complete at 96.7 min.  Calculate the half-life for this reaction.

The half-life for a first order reaction is 27min. How long will it take for 4 half-lives to occur?

For the reaction A → B, a plot of ln[A] vs. time yields a straight line with the equation y= -0.423 + 0.092x. What is the reaction order with respect to A?                                                                   What is the half-life of the reaction in (s) ?                                                                       What was the initial concentration of A (M) ?

The reaction 2 A(g) -->  A(g) obeys zero-order kinetics. The reaction begins with 5.57E2 g of A. After 8.57E0 minutes 1.93E2 g of A remains. What is the half-life for this reaction in minutes?

Determine half-life, order, and k from concentration-time data. The following data were collected for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g)-CH₂(g) + H₂(g) + CO(g) [CH3OCH 3], M 7.02x10-² time, min 0 3.51x10-2 22.20 K 1.76x10-² 44.40 8.80×10-3 66.60 (a) What is the half-life for the reaction when [CH3OCH3] = 7.02x10-² M? (b) What is the half-life for the reaction when [CH3OCH3] = 3.51x10-² M? (c) Is the reaction first order? If so, what is the rate constant for the reaction? (If not first order leave blank). min min min-1

Calculate the half life, in minutes, for a second order reaction with an initial concentration of 0.468 M and a rate constant, k, of 0.032 M-1s-1.

Given- The reaction A → B is a first-order reaction with a rateconstant of 5.87x10-4 s-1 at 485 oC.   =How long will it take for the concentration of A to decrease by 35%?=What is the half-life of this reaction?

3. It takes 42.0 min for the concentration of a reactant in a first-order reaction to drop from 0.45 M to 0.25 M at 25°C. What is the half-life for the reaction?

The decomposition of N2O5 to NO2 and O2 is first order, with a rate constant of 4.8e-4 1/s at 45°C.  Let the inital concentration of N2O5 be 1.65e-2 mol/L. What is the half-life of the reaction? How long would it take for N2O5 to decrease to 1.00e-2 mol/L from its initial value? How long would it take for N2O5 to decrease to 75% of its inital value. Sketch [N2O5] versus time