2. The decomposition of a certain insecticide in water follows first-order kinetics with a rate constant of 1.45 yr...
BREWED Name Integrated Rate Law Practice 1. The decomposition of a certain insecticide in water follows first-order kinetics with a rate constant of 1.45 yr. A quantity of this insecticide is washed into a lake on June 1, leading to a concentration of 5.0 x 10-7 M. (a) What is the concentration of the insecticide on June 1 of the following year? (b) How long will it take for the concentration of the insecticide to decrease to 3.0x 10 M?
QUESTION 19 The decomposition of a compound follows first-order kinetics with a rate constant of 1.45 y? The concentration of this compound at time = 0 was 5.0 x 10-7 g/cm3. How long does it take for the concentration of the compound to reach one-quarter of its initial value? A. 0.478 y B. 4.0 y C. 0.956 y D.351 y E. 1.39 y
The decomposition of a compound follows a first order kinetics with a rate constant of 0.0432 s^-1 at 500 degrees C. 1) if the initial concentration of starting material was 0.0500 M, what is the concentration after 1.4 min? 2) how long (in mins)will it take for the concentration of starting material to decrease from 0.750 M to 0.000250 M? 3) how long (in min) will it take to convert 32 percent of the starting material?
At a certain temperature this reaction follows first-order kinetics with a rate constant of Suppose a vessel contains at a concentration of . Calculate how long it takes for the concentration of to decrease to . You may assume no other reaction is important. Round your answer to significant digits. At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0366 s ": 250z (g) 2502(g) +0,(g) Suppose a vessel contains SO, at a concentration of...
At a certain temperature this reaction follows second-order kinetics with a rate constant of 12. M1-1 2H,PO4 (aq) + P,0, (aq) +3H,0(aq) Suppose a vessel contains H,PO, at a concentration of 1.42 M. Calculate how long it takes for the concentration of H,PO, to decrease by 92.%. You may assume no other reaction is important. Round your answer to 2 significant digits. 0 X ?
- 1 At a certain temperature this reaction follows second-order kinetics with a rate constant of 11.7 M is : 2NH3(g) → N2(g) + 3H2(g) Suppose a vessel contains NH, at a concentration of 0.670 M. Calculate the concentration of NH, in the vessel 0.510 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. x 6 ?
At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.653 M -1 -1 is : 2803 (g) → 2802(g) +O2(g) Suppose a vessel contains SO, at a concentration of 0.360 M. Calculate the concentration of SO, in the vessel 43.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. x 6 ?
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.126 s': 201,0, () - 201, ()+50,() Suppose a vessel contains CL,O, at a concentration of 1.32 M. Calculate the concentration of CIO, in the vessel 9.20 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. IM x 5 ? Submit Assignmen
The decomposition of dinitrogen tetroxide to nitrogen dioxide at 400°C follows first-order kinetics with a rate constant of 9.17 ×10-3 s-1. Starting with pure N2O4, how many minutes will it take for 85.0% to decompose?
At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.186 M−1:s−1 2NH3g -> N2g + 3H2g Suppose a vessel contains NH3 at a concentration of 0.440M. Calculate how long it takes for the concentration of NH3 to decrease by 77.0%. You may assume no other reaction is important. Round your answer to 2 significant digits.