1:16 Sun, 16 June bb. = University of South Australia Dashboard SP2 2024 Chemistry 100 Dashboard > CHEM 1006 > Online Quizzes Online quiz 4 Question 2 The data in the table below were obtained for the reaction: Incorrect Course Outline + Mark 0.00 out of 1.00 NO2 + 03 → NO3 + 02 Content Flag question Use the data shown to determine the rate law for the reaction. Experiment Number [NO2] (M) [03] (M) Initial Rate (M/s) Academic 1 0.21 0.70 6.30 x 10-3 Integrity 2 0.63 0.70 1.89 x 10-2 3 0.21 0.35 3.15 x 10-3 Assessment 4 0.42 0.35 6.30 x 10-3 Grades Ө Extensions 미이 이미 Resources What is the overall order of the reaction? a. rate = k [NO2][03] b. rate = k [NO₂]²[03] x c. rate = k [NO2][03]² d. rate = k [NO₂2] Recordings e. rate = k [NO3][02]/[NO2][03] *༢ དཱི51% 10 ? Yunseo Kwon 16 Ob Sunday, 16 June 2024 1:16 am ACST = • о < ←

Use the data presented in the table to determine the rate equation for the hypothetical reaction shown. A(g) + 2B(g) + 3C(g) [Math Processing Error] D(g) + 2F(g) Exp {A} (M) {B} (M) {C} (M) initial rate (M/min) 0.0025 0.0025 0.0025 3.16x10-11 0.0025 0.0050 0.0025 1.27x10-10 3 0.0050 0.0050 0.0025 1.27x10-10 4 0.0100 0.0100 0.0050 4.06x10-9 What is the reaction order with respect to A? What is the reaction order with respect to B? What is the reaction order with respect to C? Enter each of your answers numerically as integers or fractions (ex: 0, 1/2, 1, 3/2, 2, 3, etc). Hint: Determining the order of one of the reactants will be difficult. Determine the order of the two easy reactants first, then use that information in determining the difficult one.

Hi! Please use the graph in the question to answer part a!

1:18 Sun, 16 June bb. = University of South Australia Dashboard Course Outline Content Academic Integrity Assessment In Grades Ө SP2 2024 Chemistry 100 Dashboard > CHEM 1006 > Online Quizzes > Online quiz 4 Question 4 If the rate law for the reaction Correct Mark 1.00 out 2A + 3B → products of 1.00 Remove flag is first order in A and second order in B, then the rate law is rate = a. k[A][B] b. k[A][B]² c. K[A]²[B]² d. k[A][B] e. k[A]²[B] Extensions Resources Your answer is correct. The correct answer is: k[A][B]² Recordings 16 b *༢ དཱི51% 10 ? Yunseo Kwon = ||| о Sunday, 16 June 2024 1:18 am ACST ←

O https://app.101edu.co A * Question 7 of 20 Determine the rate law for the reaction A+ B - C + D given the following experiment data. Initial Trial [A]o [B]o Rate A) Rate = k[A] %3D (M/min) B) Rate = k[A]? 1 0.25 0.40 7.25 C) Rate = k[A][B] %3D 2 0.75 0.40 21.5 D) Rate = k[A]°[B] %3D 3 0.50 0.80 14.5 E) Rate = k[A][B] 4 0.75 0.80 21.5 Delete F12 wwwn D F11 FI0 FO FB FS FO Backspace Num Lock F2 %3D 1 8. 6. 4 12 3 Wome E R Enter J K F S. Shift Poyblip Ctr Alt Home All

Calculate the concentration [A] for a reaction A Product after 7.00 min, knowing that the initial concentration [A]o is 2.4 M, and the rate constant is 3.2x10-3 M-1sec-1. Edit Format Table 12pt v Paragraph v BIU T?v : hp 732006020610 f3 米 fo f9 @

D. Pls answer asap . Pls provide accurate answer. Help me thank uuu. Handwritten thank u.

Consider a reaction: A+ B → C and the rate law expression: Rate = k [A]M[B]^ %3D In the rate law expression above, what do 'm' and 'n' determine? order of reaction concentration of A and B they have no significance I have no idea