Question

02 Question (4 points) Dinitrogen pentoxide (N2O) decomposes as follows to nitrogen dioxide and nitrogen trioxide: N205(8) ► NO2(g) + NO3 (8) Calculate the average rate of the reaction between consecutive measurement times in the fbllowing table. Time (s) (N2O5] (molecules/cm) 0.00 1.605x1012 1.45 1.526x1012 2.90 1.465x1012 4.35 1.416x1012 5.80 1.377x1022 1st attempt 3 OF S QUESTIONS COMPLETED < 02/05 >

Answer 1

Reaction : NO ( No (8) + NO3(a). Table Time(s) 0.00 [Nos (molecules/cms) | 1.605 X 1012 1-526 X 102 1.465 x 102 1.416 x 10² 1.45 2.90 4.35 5.80 1.377 x 10² Average rate = decrease in concentration of No Time taken. Rate I = (1.605x10² - 1.526x102) (1.45 -0.00) 12 Rate L = 0.054 x 10" ñ 0.05 x 10 moleads/com

TU Rote 2 = COS ರ್ವಜನಿಕ ಶಿಕ್ಷಣ ಇಲಾಖೆ, " (1.526x102 - 1.465X102) (2.90 - 1.45) 0.042 X 10th molecules/cms) = 0.04X10² Rate2 = Rate 3 = (1.465 x 102 - 1.4 16x102) (4.35 - 2.90) Rate 3 = 0.034 X10 moleculey /enes | 2 0.03410² Rate u = (1.416% 10² - 1.37781012) (5.80- 4.35) Rate 4 = 0.027 x 10 moleculy /con.sl~ 0.03 010² & In order to show that the concentration of No decrease through out the reaction , negative sign can be used for the rate.

in the above question, it is asked to determine the average rate for the decomposition reaction of N2O5

in the table the time taken for the decomposition is given in the intervals of 1.45sec and the corresponding concentration of N2O5 is also given.

the average rate can be defined as the ratio of the change in the concentration of the chemical substance to the time taken .

that is, average rate = ( change in concentration of chemical substance ) / time taken

in this case , average rate = (decrease in concentration of N2O5) / time taken