The decomposition of N2O5 can be described by the equation 2N₂O₂(soln) - 4 NO2 (soln) + O2(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. (s) 0 [N2O5] (M) 1.849 145 1.688 416 1.423 745 1.157 Given the data, calculate the average rate of reaction for each successive time interval. What is the average rate of reaction for the time interval from 0s to 145 s? 1.11 ×10¯³ -3 average rate of reaction: Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books M/s of 19 > average rate of reaction: 1.11 ×10−3 Incorrect What is the average rate of reaction for the time interval from 145 s to 416 s? 9.78 ×10-8 average rate of reaction: Incorrect What is the average rate of reaction for the time interval from 416 s to 745 s? average rate of reaction: 8.09 ×10-4 Incorrect > Attempt 1 M/s M/s 123 Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry | Publisher: University Science Books ::

Consider following reaction:              2 A2B5(g)  →  4AB2(g) + B2(g) The rate constant is 0.129 s-1 at 298 K for this reaction. What is the percent of A2B5 left after the first 19.091 s? Report your answer with three decimals. Enter numbers only;

A chemical engineer is studying the rate of this reaction. 2N,O; (g) → 2N,O4 (g) +O, (g) He fills a reaction vessel with N,O, and measures its concentration as the reaction proceeds. Here's a graph of his data: 0.8 0.6 0.4 0.2. 20 40 60 80 100 t (s) (W)['o°N]

The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH3(g) + 302(g) → 2N2(g) + 6H₂O(A) Suppose the rate of formation of H₂O(A) is 3.0 mol/(Ls). Which of the following statements is true? The rate of consumption of NH3 is 2.0 mol/(L. s). The rate of consumption of O₂ is 2.0 mol/(L. s). The rate of formation of N₂ is 1.3 mol/(Ls). The rate of formation of N₂ is 2.0 mol/(Ls). The rate of consumption of NH3 is 0.50 mol/(L. s).

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 = 2.47 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)

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 = 2.55 x 108 s 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 overall reaction of ozone reacting to form oxygen has been proposed to occur in a reaction mechanism of: Step 1: O3(g)-→O2(g) + O(g) Step 2: O3(g) + O(g) →202(g) What is the role of O(g) and what is the overall balanced equation? Periodic Table and Datasheet Select one: O a. O(g) is an intermediate; 203(g) + O(g) →302(g) + O(g) O b. O(g) is a catalyst; 203(g) + O(g)→302(g) + O(g) O c. O(g) is an intermediate; 203(g) → 302(g) O d. O(g) is a catalyst; 203(g)→302(g) Which statement best describes general equilibrium?

I completed the problem but for some reason, my answer is still wrong. for part a I got 5.48 x 10^-5 and for part b I got 5.61x10^-4. I substituted the concentrations in the equation but hey still seem to be wrong can someone explain?

Consider this reaction: →NH4OHaq+NH3aqH2Oaq At a certain temperature it obeys this rate law.rate =·26.0M−1s−1NH4OH2 Suppose a vessel contains NH4OH at a concentration of 1.28M. Calculate the concentration of NH4OH in the vessel 0.270 seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits. =___M

At a certain temperature the rate of this reaction is first order in H₂CO3 with a rate constant of 4.73 s H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 1.01 M. Calculate how long it takes for the concentration of H₂CO3 to decrease to 0.212M. You may assume no other reaction is important. olo Round your answer to 2 significant digits. B s ?