Question 9In the reaction below, using the following data, determine the rate law for the following reaction:NH,° (aq) + NO,"(aq) → N;(g) +2 H,O)Experiment[NHI (M)[NO2] (M)Rate (M/s)0.25000.25001.250 x 10-30.50000.25002.500 x 10-30.25000.12503.125 x 10 -4Oa. K[NH4 J[NO2Ob.K[NH4 J[NO27/2OC. KINH47²INO2Od. KINH4 INO2O e. KINH41/2[NO27MacBook AirSC吕口F3888F4F1F2F5F6F7F8F9F10F11232$&234578TYQER

Answered: Image /qna-images/answer/8ba4f660-6643-4d22-82fb-4254ab51204e.jpg

Question 9 In the reaction below, using the following data, determine the rate law for the following reaction: NH, (aq) + NO,"(ag) → N,(8) +2 H,O() Experiment [NH41 (M) 0.2500 Rate (M/s) [NO27 (M) 0.2500 1 1.250 x 10 -3 2.500 x 10 -3 3.125 x 10 -4 2 0.5000 0.2500 3 0.2500 0.1250 Oa. KINH4[NO2Y Ob.K[NH4 J[NO2772 OC. KINH4INO27 Od. K{NH4 [NO2] Oe. KINH4/2NO2

Question 9 In the reaction below, using the following data, determine the rate law for the following reaction: NH, (aq) + NO,"(ag) → N,(8) +2 H,O() Experiment [NH41 (M) 0.2500 Rate (M/s) [NO27 (M) 0.2500 1 1.250 x 10 -3 2.500 x 10 -3 3.125 x 10 -4 2 0.5000 0.2500 3 0.2500 0.1250 Oa. KINH4[NO2Y Ob.K[NH4 J[NO2772 OC. KINH4INO27 Od. K{NH4 [NO2] Oe. KINH4/2NO2

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

the data in the table below were obtained for the reaction (see image) what is the magnitude of the rate constant for the reaaction
Give only typing answer with explanation and conclusion
Using the data in the table, determine the rate constant of Trial [A] (M) [B] (M) Rate (M/s) the reaction and select the appropriate units. 1 0.280 0.200 0.0163 A +2B C+ D 0.280 0.400 0.0163 0.560 0.200 0.0652 Units k =
I need the answer as soon as possible
QUESTION 7 (PC) Use the data provided below to determine the value of the rate constant for the reaction 4 A(aq) + 3 B(g) products. exp Initial [A] Initial [B] Initial rate (M/min) 0.010 0.120 1.224x10-6 0.020 3.332х10 6 6.528×10-6 0.140 3. 0.030 0.160 4. 0.040 1.360×10-5. 1.020×10¬5 0.200 5. 0.030 0.200 0.060 0.220 2.4684×10-5
2) Can some one explain the question
Consider the following complex reaction: P + 2Q → Products whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [P](M) [Q](M) Rate(M/s) 1 0.100 0.050 2.25 × 10−3 2 0.100 0.150 6.75 × 10−3 3 0.200 0.050 9.00 × 10−3 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law (express your answer to three significant figures), and select the units for k.
Using the data in the table, determine the rate constant of the Trial [A] (M) [B] (M) Rate (M/s) reaction and select the appropriate units. 1 0.220 0.210 0.0157 A + 2B C+D 0.220 0.420 0.0157 3 0.440 0.210 0.0628 Units k = M-ls-1 M-2s-1 M-s-1
For the reaction 2A + B2→ 2AB, the following information was obtained: Trial [A](M) [B](M) Initial Rate (M/s) 1 1.5 2.0 0.183 2 4.0 3.0 1.098 3 3.0 4.5 1.863 4 1.5 4.0 0.732 5 4.5 2.0 0.549 Determine the rate law and calculate the value of the rate constant. You must justify your answers.
Please show all steps in the question attached, right answer 1,1
Consider the following complex reaction: A + 2B → C whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [A](M) [B](M) Rate(M/s) 1 0.400 0.050 9.60 × 10−3 2 0.400 0.100 1.92 × 10−2 3 0.800 0.050 3.84 × 10−2 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law. Express your answer to three significant figures. Include units for k.
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