In the first-order decomposition of cyclobutane, it is found that 25% of the sample has decomposed after 80 seconds. What is the half-life (t 1/2) of the reaction? (ln([A] t /[A] 0 )= -kt; t 1/2 =0.693/k)

Given the following data, determine the rate law for the reaction 2 NO(g) + O2g)22 NO2(g) Experiment [NO] (M) [O2] (M) Rate (M/s) 1 0.0300 0.0200 3.6 x 10-4 2 . 0.0600 0.0200 7.2 x 10-4 3 0.0600 0.0400 14.4 x 10-4 a) Determine the order of the reaction for each reactant, N, and 02. b) Write the rate law rate equation. ' ) ) Determine the value of the rate constant. (

If the decomposition of reactant A follows first-order kinetics, what concentration of A remains if [A], = 0.273 M, k = 1.53 × 10-2 minutes-1, and the elapsed time = 1.61 hr? A) 0.009 M B) 0.273 M c) 0.109 M D) 0.0623 M

The thermal decomposition of PH3 is a first order process: 4 PH3(g) P4(g) + 6 H2(g) If the value for the rate constant, k equals 2.00 x 10/sec, how long (sec) would it takes for 85% of the PH3 to decompose? Express the answer to 3 sig. figs. In[A]t = -kt + ln[A]o sec

A second-order decomposition reaction run at 550°C has a rate constant of 7.1 x 10L/(mol -s). If the initial concentration of the reactant is 0.10 M, what is the concentration of this reactant after 1.4 x 10 s? What is the half-life of this reaction under these conditions? Concentration = м IHalf-life =