Remaining* Question Completion Status:A Moving to another question will save this response.Question 9Consider the following reaction that follows a second order rate law.2 NO2 (g) → 2 NO (g) + O2 (g)If (NO2]o = 0.0500 M and k = 0.543 M-1s-1, then what would be the concentration of NO2 after 1800 seconds?O 5.68 x 10-3 MO 1.77 x 10-3 MO 1.00 x 10-3 MO 2.05 x 10-3 MO 4.51 x 10-3 MA Moving to another question will save this response.MacBook Airesc20FIF2F3F5F6#3$4&4.QER.Y.ASH.LL3.w/

Answered: Image /qna-images/answer/1f70c778-e0fe-4b82-97f9-82f76c63940a.jpg

Question 9 Consider the following reaction that follows a second order rate law. 2 NO2 (9) →2 NO (g) + O2 (g) If (NO210 = 0.0500 M and k = 0.543 M-1s-1, then what would be the concentration of NO2 after 1800 seconds? %3! %3D O 5.68 x 103 M O 1.77 x 103 M O 1.00 x 103 M O 2.05 x 103 M O 4.51 x 103 M

Question 9 Consider the following reaction that follows a second order rate law. 2 NO2 (9) →2 NO (g) + O2 (g) If (NO210 = 0.0500 M and k = 0.543 M-1s-1, then what would be the concentration of NO2 after 1800 seconds? %3! %3D O 5.68 x 103 M O 1.77 x 103 M O 1.00 x 103 M O 2.05 x 103 M O 4.51 x 103 M

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Question 3 only
The rate of a certain reaction is given by the following rate law: rate=k H2 | I2| *[H:]L] Use this information to answer the questions below. What is the reaction order in H,? What is the reaction order in I,? ? What is overall reaction order? At a certain concentration of H2 and I2, the initial rate of reaction is 34.0 M / s. What would the initial rate of the reaction be if the concentration of H2 were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 0.530 M/ s when [H2] = 1.4 M and [I2] = 0.21 M. Calculate the value of the - 1 - 1 k = |M •S rate constant. Round your answer to 2 significant digits.
The rate of a certain reaction is given by the following rate law: rate =k N, O, Use this information to answer the questions below. olo What is the reaction order in N,? |x10 18 Ar What is the reaction order in 03? What is overall reaction order? At a certain concentration of N, and 03, the initial rate of reaction is 0.780 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 5.0 x 103M/s when [N2] = 1.1 M and [03] = 1.1 M. Calculate the value of - 3 -1 k = |M •S the rate constant. Round your answer to 2 significant digits.
Consider the reaction: H2 (g) +I2 (g) → 2 HI (g) A chemist performed an experiment and monitored the concentration of I2 during the course of the reaction. The red line in the graph below represents the results obtained. Which line in the plot would best represent how the concentration of HI changes during the course of the reaction? Time (s) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a a b b d d е е Concentration (M)
Question is attached.
Please show all steps in the question attached, right answer 1,1
The data below were collected for the following reaction: CH3CI(g) + 3 Cl2(g) CCI4(g) + 3 HCI(g) [CH3CI] / mol L-1 Initial Rate / mol L-1 s-1 Trial [Cl2] / mol L-1 1 0.050 0.050 0.0142 2 0.100 0.050 0.0290 3 0.200 0.200 0.115 What is the order of the reaction with respect to Cl2?
The rate of a certain reaction is given by the following rate law: =k[N₂]²[H₂]² Use this information to answer the questions below. rate What is the reaction order in N₂? What is the reaction order in H₂? What is overall reaction order? At a certain concentration of N₂ and H₂, the initial rate of reaction is 71.0 M/s. What would the initial rate of the reaction be if the concentration of N₂ were halved? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 0.930 M/s when [N₂] = 0.79 M and [H₂] = 0.88 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. M 04/1 S -3 1 k = M ²³.5²¹ S
Help with the question on the right Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, find the rate law. 0–H (RCOOH), M [R'OHJ, M (HAJ, M Initial Rate, M-min"' - R-C+ k2 R С—0—Н + HA A- 0.35 0.35 0.50 4.60 0.50 0.62 0.35 0.35 8.14 0.81 0.50 10.6 0.35 0.50 0.75 0–H 9.84 Group 1 0–H 0–H k3 Rate = k[RCOOH][R'OH] R-Ć+ A- R 0–H R—С—0—Н + Rate = k[RCOOH][R'OH][HA] k4 0–H R-ó+ A- Group 2 Rate = k[RCOOR']/{[RCOOH][R'OH]} H Rate = k[R'OH] 0–H Rate = k[RCOOH] k5 R- C-0–R' R-C-0–H + H,о + НА R-o+ A- Group 3 Step 2 or Step 3 O Step 1 or Step 2 Step 1 Step 3 Step 2 Step 1
The rate of a certain reaction is given by the following rate law: ₂= k[N₂][H₂]² Use this information to answer the questions below. rate= What is the reaction order in N₂? What is the reaction order in H₂? What is overall reaction order? At a certain concentration of N₂ and H₂, the initial rate of reaction is 0.090 M/s. What would the initial rate of the reaction be if the concentration of N₂ were doubled? Round your answer to 2 significant digits. The rate of the reaction is measured to be 45.0 M/s when [N₂] 1.0 M and [H₂] = 0.48 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. 0 k = 04/1 = M². x10 X