Why is it divided in half? I always thought we just plug it into the found rate. That's what I did with the others, and those were right. What's different?

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Consider the graph below. Time If the equation of the line above has a slope of 1.911 and intercept of 8.747, what is the initial concentration of A? 1/[A]

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…

537 of 5 33. The decomposition of nitrosyl chloride was studied: 2NO(g) + Cl₂(g) 2NOCI(g) The following data were obtained where A[NOCI] Copyright 2018 Cengage Learning. All Rights Reserved. May not be copied, scanned, or duplicated, in whole or in part. Rate = [NOCI], (molecules/cm³) 3.0 × 10¹6 2.0 × 10¹6 X 1.0 X 10¹6 4.0 × 10¹6 Initial Rate (molecules/cm³-s) 5.98 × 104 2.66 X 10* 6.64 × 10³ 1.06 × 10³ 0.060 a. Determine the rate law. b. Calculate a value for the rate constan and an average value for the rate con a. What is the rate law? b. Calculate the value of the rate constant. c. Calculate the value of the rate constant when concentra- tions are given in moles per liter. 0.030 34. The following data were obtained for the gas-phase decompo- sition of dinitrogen pentoxide, 2N₂O₂(g) → 4NO₂(g) + O₂(g) 36. The reaction 2NO(g) + was studied, and the follo [NO] (molecules/cm³) 1.00 X 10¹8 3.00 × 1018 2.50 X 10¹8 Ra [ (molec 1.00 1.00 2.50 What would be the in [NO] 6.21 x 10¹8 1018…

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Problem 2 Consider the following reaction between nitrogen dioxide gas and carbon monoxide gas 21 + 2H* + H2O2 → I2 + 2H20 (g) The experimentally determined rate law for this reaction is Rate = k [I"] [H2Oz]. The following mechanism has been proposed I + H2O2 → HOI + OH" HOI + I → OH" + I2 (g) Slow Fast H* + OH" → H2O Fast

The liquid phase reaction A + 0.5B → C is first order in A and first order in B, and second order overall. Starting with an equimolar mixture, the reaction goes to 20% completion in 500 seconds. (Although CAo is not needed to solve the problem, for simplicity use CA0 = 1 mol/m³ for all parts) a. Is A or B the limiting reactant? b. Calculate the conversion of A and B. c. Plot the concentrations (CA/CA0 and CB/CA0, Cc/CA0) and rate of formation of C as a function of time. d. Plot the concentrations as a function of time if the reaction is first order in A and half order in B.

A group of students compiled the data shown in data table 1 below.  What is the exact calculated order for H+(aq) to 2 decimal places? Exp. # [IO3-]0 (M)   [I-]0 (M)    [H+]0 (M) Time (s) 1 0.005 0.05 2 x 10-5 22.12 2 0.010 0.05 2 x 10-5 86.84 3 0.005 0.10 2 x 10-5 5.35 4 0.005 0.05 4 x 10-5 2.65     Question 6 options:   2.82   -2.51   3.34   2.71   -2.58   3.12   2.91   3.49   3.41   3.23   3.06   2.64

question b is where i am having trouble with !