Consider the reaction A + 2B = C Part A whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: What is the rate law for this reaction? [A] | [B] (M) (M) (M/s) Rate Express the rate law symbolically in terms of k, [A], and [B]. Trial • View Available Hint(s) 0.20 0.050 2.4x10-3 2 0.20 0.100 4.8×10¬3 rate = k[A]° [B] 3 0.40 0.050 |9.6x10¬3 Submit Previous Answers Correct Part B Calculate the initial rate for the formation of C at 25 °C, if [A] = 0.50 M and [B = 0.075 M. Express your answer to two significant figures and include the appropriate units. • View Available Hint(s) initial rate = Value Units Submit Provide Feedback

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A) Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3-  -->  4 Zn2+ + N2O(g) + 5 H2O(l) What is the rate law for this reaction? Group of answer choices rate = k [H+][NO3-] rate = k [H+]10[NO3-]2[Zn2+]4[N2O] More information is needed to determine this. rate = k [H+]10[NO3-]2   B) Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3-  -->  4 Zn2+ + N2O(g) + 5 H2O(l) If the rate of H+ disappearance is 0.0250 M/min, what is the rate of Zn2+ appearance? Group of answer choices 0.0100 M/min 0.00100 M/min 0.0250 M/min 0.0625 M/min

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 ←

Explain your reasoning, please. Thank you.

The integrated rate laws for zero-, first-, and second-order reaction may be arranged such that they resemble the equation for a straight line, y = mz +b. • Part A Order Integrated Rate Law Graph Slope [A] =- kt + [A]Jo -kt + In[A]o In[A] vs. t + = kt + TAT [A] vs. t -k The reactant concentration in a zero-order reaction was 7.00x102 M after 170 s and 3.00x102 M after 380 s. What is the rate constant for this reaction? 1 In[A] = -k Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash. 1 - vs t JA 2 • View Available Hint(s) ? koih = Value Units Submit Prevlous Anawera Part B Complete previous part(s) • Part C The reactant concentration in a first-order reaction was 6.60x102 Mafter 30.0 s and 7.70x10 Mafter 100 s. What is the rate constant for this reaction? Express your answer with the appropriate units. Indicate the multiplication of units, as necessary, explicitly either with a…

Consider the following complex reaction:   2NO2(g) + O3(g) →  N2O5(g) + O2(g) whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [NO2](M) [O3] (M) Rate (M/s) 1 0.20 0.40 0.25 2 0.40 0.40 0.50 3 0.40 1.20 1.50    What is the rate law for this reaction? Write the value for k to two significant figures in the first box. Select the units for k and concentration terms in the second box.

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