masteringchemistry.com/myct/itemView?assignmentProblemlD=135892239 CHEM 1212 Spring 2020 <1212 - Ch 14 B ± Experimental Determination of a Rate Law Review Consider the reaction A+2B C Part B whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Calculate the initial rate for the formation of C at 25 °C, if A = 0.50 M and B=0.075 M [A] B] Rate Trial (M) (M) (M/s) Express your answer to two significant figures and include the appropriate units. 1. 0.15 0.050 1.4x10-3 > View Available Hint(s) 0.15 0.100 2.7x10-3 3 0.30 0.050 5.4x10-3 HA initial rate =2.3 10 2 m•s-1 Submit Previous Answers X Incorrect; Try Again; 3 attempts remaining Provide Feedback Type here to search Chp 2. II

masteringchemistry.com/myct/itemView?assignmentProblemlD=135892239 CHEM 1212 Spring 2020 <1212 - Ch 14 B ± Experimental Determination of a Rate Law Review Consider the reaction A+2B C Part B whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Calculate the initial rate for the formation of C at 25 °C, if A = 0.50 M and B=0.075 M [A] B] Rate Trial (M) (M) (M/s) Express your answer to two significant figures and include the appropriate units. 1. 0.15 0.050 1.4x10-3 > View Available Hint(s) 0.15 0.100 2.7x10-3 3 0.30 0.050 5.4x10-3 HA initial rate =2.3 10 2 m•s-1 Submit Previous Answers X Incorrect; Try Again; 3 attempts remaining Provide Feedback Type here to search Chp 2. II

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...

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Question 4 Calculate the frequency factor (A). Studies have shown that the reaction occurs via the following mechanism. ki Cl2O4 k-1 Step 1: 2 Cl02 (fast equilibrium) k2 Step 2: C2O4 + OH- → ClO;¯+HCIO2 (slow) k3 Step 3: HCIO2 + OH → ClO2¯+H2O (fast) Question 5: Identify the intermediate/s and the rate-determining step. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 → ClO3¯+HC1O2 Step 2: C204 + OH- (slow) k3 Step 3: HC1O2 + OH- ClO2- + H2O (fast) Question 6 Is the proposed mechanism consistent with the experimentally determined rate law? Show your solution to justify your answer. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 Step 2: C204 + OH- → ClO3¯+ HCIO2 (slow) k3 Step 3: HCIO2 + OH- → ClO2-+ H2O (fast) Question 7 Draw the transition state for Step 3. Identify the bond/s forming/breaking.
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Write rate law for the chemical reaction ?
Q4
The reaction 2 N205(g) → 4 NO2(g) + O2(g) was studied and the rate of change of the concentration of O2 was found to be 3.65 mol L 15-1. Calculate the reaction rate (in mol L1s1). Reaction rate = i mol L-1s-1. eTextbook and Media Save for Later Attempts: 0 of 3 used Submit Answer
The overall gas phase reaction 3A --> B + 2C occurs via the following sequence of elementary steps 2A <--> I1 + B k1,k2 A + I1 --> 2I2 k2 I2 --> C k3 1. write an expression for the overall reaction rate, r, in terms of the rate step 3, r3 2. using the answer from 1, obtain an expression for the reaction rate, r, in terms of rate constants and concentrations of reactants and products, only use PSSH. 3. State the. specific inequality the must be satisfied for each of the following assumptions to hold, and use it to simplify the general rate expression from question 2. i) Step 1 is quasi-equilibrium ii) Step 1 is irreversible
The following data were obtained for the hypothetical reaction: The proper units of the rate constant should be: The data necesary is in the image
A Moving to another question will save this response. Question 24 The rate law for the reaction below is rate = k[N21*[H2]Y 2 NH3 N2 + 3 H2 - Which of the following is true? OA.x = 3 and y = 1 OB. The reaction is 4tn order overall OC The order of reaction needs to be determined experimentally O D.X = 1 and y = 1 OE.x = 1 and y = 3 A Moving to another question will save this response. MacBook esc F1 F2 F4 FS 23 3 4. tab aps lock F
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 @
A reaction between the substances A and B (3A + 2B2 ⟶ 2C + D) gives the following data:
Given that the rate constant for the decomposition of hypothetical compound XX from part A is 1.60 M−1⋅min−1�−1⋅min−1, calculate the concentration of XX after 13.0 minmin .