### Part CWhat is the rate law for step 1 of this reaction?**Express your answer in standard MasteringChemistry notation. For example, if the rate law is \( k[A][C]^3 \), type k\*[A]\*[C]^3.**- **View Available Hint(s)** **Rate =** [Input box]**Submit [Button]**---### Part DWhat is the rate law for step 2 of this reaction?**Express your answer in standard MasteringChemistry notation. For example, if the rate law is \( k[A][C]^3 \), type k\*[A]\*[C]^3.**- **View Available Hint(s)** **Rate =** [Input box]**Submit [Button]** **Order and Rate Law of a Reaction**The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is \[ \text{rate} = k[\text{NO}_2]^2 \]The exponent "2" is used because the reaction involves two NO₂ molecules. The rate law for step 2 is \[ \text{rate} = k[\text{NO}_3]^1 [\text{CO}]^1 = k[\text{NO}_3][\text{CO}] \]because the reaction involves only one molecule of each reactant the exponents are omitted.**Analyzing a New Reaction**Consider the following elementary steps that make up the mechanism of a certain reaction:1. \( 3A \rightarrow B + C \)2. \( B + 2D \rightarrow C + F \)**Part A**What is the overall reaction? *Express your answer as a chemical equation.*[View Available Hint(s)]

Given : 3A --> B +C B + 2D --> C +F

Part C What is the rate law for step 1 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C] type k*[A]* [C]^3. > View Available Hint(s) Rate = Submit Part D What is the rate law for step 2 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C3 type k*[A]* [C]^3. > View Available Hint(s) Rate =

Part C What is the rate law for step 1 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C] type k[A] [C]^3. > View Available Hint(s) Rate = Submit Part D What is the rate law for step 2 of this reaction? Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C3 type k[A] [C]^3. > View Available Hint(s) Rate =

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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9. Write a generic rate law for each line in the graph below and give the appropriate units of k for the graphs below. Rate Mos-1 (2) (3) [A] 10. Convert the integrated rate law for a 1st-order reaction to the slope-intercept form and draw a general graph making sure to identify the y-intercept, slope, x-intercept (with appropriate labels), and label the y- and x-axes with the appropriate labels.
2. Imagine you run a reaction whose free energy of activation (AG*) is 18 kcal/mol. If it were a first order reaction, its’ half life (the time for half the starting material to go away) or half the product to form (assuming a 100% yield) would by In2/k where k is the rate constant. How long will it take for the reaction to be done if you run the reaction in an ice-salt bath at room temperature (20 °C) if the rate constant were 1 x 104/sec?
Please help me.
We are determining the rate law equation for a reaction A + B + C > ABC in which a dramatic and instant color change tells us that reactants are used up and product is formed. (Concentrations used in all experiments are [A] = 2.0M, [B] = 1.0M and [C] = 3.0M) This is the data for questions 19 through 22: Volume of Volume of water, C, Volume of Volume of Time from mixing to dramatic color А, B, ml change, sec ml ml ml 1.0 1.0 1.0 97.0 16 1.0 1.0 2.0 96.0 8 19) Which reactant concentration have we changed? a) A b) B c) C d) no reactant concentrations changed
Learning Goal: To understand zero-order reactions. Chemical kinetics is the study of the speed with which a chemical reaction occurs and the factors that affect this speed. The speed of a reaction is the rate at which the concentrations of reactants and products change. This relationship is expressed through rate laws. For a general reaction aA + bBgG+ hH, the rate law is given as rate of reaction= k[A] [B]" where the coefficients and are experimentally determined while a, b, g, and h are stoichiometric coefficients unrelated to me and n Azero-order reaction has a rate law in which the sum of the exponents m +n + ... is equal to zero. Thus, if there is only one reactant, the rate of reaction is independent of the concentration of the reactant. For a zero-order reaction, the graph of reactant concentration versus time is a straight line. Therefore, the rate-law equation for a zero-order reaction can be compared to that of a straight line, y = mz+b ✓ Correct Important: If you use this…
18. Derive the rate law for the following multi-step reaction: CH4 + OH = CH3 + H2O (fast) CH3 + O2 = CH3O2 (fast) CH3O2 → CH2OOH (slow)
Would this be the correct answer ?
I Review | Constants | Period MISSED THIS? Read Section 15.4 (Pages 642 - 649); Watch KCV 15.4, IWVE 15.4.The decomposition of SO2 Cl2 is first order in SO2 Cl2 and has a rate constant of 1.40x104s-1 at a certain temperature. -kt + In(SO2C2]o - (1.40 x 10-s)(220 s) + In 0.175 M In[SO2 Cl2]t %3D -1.774 Take the inverse natural logarithm of both sides of the equation. [SO2 Cl2]: e-1.774 M 0.170 M Part E If the initial concentration of SO2 Cl2 is 0.175 M, what is the concentration of SO2 Cl2 after 510 s ? Express your answer using three significant figures. ΑΣφ (SO2 Cl2]e = M
5. What is the value for the rate constant, k? k = k'/1* = k = k"/0.5* = kavg r = k[OH°]*[ C25H3„N,'J" [OH] C2H,„N;'] r = 303