According to the reaction below, initial reaction rate was measured at different initial concentrations of HCI. Suggest a reaction rate expression like - HCIO = KCHCI 4HCI+ CaMg(CO3)2 Mg 2+ 2+ + Ca + 4Cl + 2CO2 + 2H2O CHCI,O, (mol/cm³) 1 4 2 0.1 0.5 -THCI,O, (mol/s) x 107 1.2 2 1.36 0.36 0.74

According to the reaction below, initial reaction rate was measured at different initial concentrations of HCI. Suggest a reaction rate expression like - HCIO = KCHCI 4HCI+ CaMg(CO3)2 Mg 2+ 2+ + Ca + 4Cl + 2CO2 + 2H2O CHCI,O, (mol/cm³) 1 4 2 0.1 0.5 -THCI,O, (mol/s) x 107 1.2 2 1.36 0.36 0.74

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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Smail ||| YouTube O KINETICS AND EQUILIBRIUM Using an integrated rate law for a first-order reaction At a certain temperature the rate of this reaction is first order in NH4OH with a rate constant of 0.0108 s NH,OH(aq). } → NH, (aq) +H,O(aq) Translate M Suppose a vessel contains NH4OH at a concentration of 1.24 M. Calculate the concentration of NH OH in the vessel 63.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. Explanation 82°F Mostly cloudy Check 0/5 Q Search © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | 1
An experiment was carried out to investigate the effect of concentration on the reaction: BrO3(aq) + 5 Br (aq) + 6 H* (aq) = 3 Br₂ (1) + 3 H₂O (1) The following data was obtained: Initial [BrO3] Initial [Br] Initial [H*] Initial Rate Trial (mol/L) (mol/L) (mol/L) (mol/L's) 1 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.20 0.20 0.10 3.2 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 a) Deduce and state the rate law equation for this reaction. Show your process/reasoning. b) Calculate the value of k, the rate constant with correct units.
The integrated rate law is an equation that describes the concentration of a reactant over time (t). The integrated rate law comes in different forms depending on the reaction order. The rate laws below are given for a simple general reaction A-products Order 0 1 2 Integrated rate law [A] = -kt+ [A]o In[A] = − kt+In[A]o =kt+ [A]o Linear graph Slope [A] vs. t -k In[A] vs. t -k V vs. t k
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
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Question 9 of 36 Submit What is the rate at which Br"(aq) disappears in the reaction below if the rate of disappearance of BrO3 (aq) is 0.020 M/ s? BrOg + 5 Br + 6 H* → 3 Br2 + 3H20 | M/s 1 2 3 4 C 7 9 +/- х 10 0 LO 00
If the y-axis of the graph changes to “volume of hydrogen / cm3 ”, sketch this rate curve. What will be the effect on the reaction rate if the concentration of HCl changes from 0.1 M to 0.2 M? Explain
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A reaction profile (not to scale!) for the reaction СН,Br + OH —С,H;ОН + Br →C¿H5OH + Br is shown below: Е (kJ) 90 C2H5BR + OH" 71 C2H5OH + Br* Reaction Coordinate This reaction is (exothermic,endothermic) The value of the activation energy for this reaction is kJ and the value of AE is kJ.
Use the provided initial rate data to derive the rate law for the reaction whose equation is: OCI (aq) + (aq) → OI¯¯(aq) + Cl¯¯(aq) Trial [OCI-] (mol/L) 1 0.0040 2 0.0020 3 0.0020 [I-] (mol/L) Initial rate (mol/L sec) 0.0020 0.00300 0.0040 0.00450 0.0020 0.00675 Determine the rate law expression and the value of the rate constant k with appropriate units for this reaction.
Help with the question on the right Question 23 Identify the rate-determining step based on the rate law you found in question 23. Given these data for the acid-catalyzed reaction in question 22, find the rate law. 0–H (RCOOH), M [R'OHJ, M (HAJ, M Initial Rate, M-min"' - R-C+ k2 R С—0—Н + HA A- 0.35 0.35 0.50 4.60 0.50 0.62 0.35 0.35 8.14 0.81 0.50 10.6 0.35 0.50 0.75 0–H 9.84 Group 1 0–H 0–H k3 Rate = k[RCOOH][R'OH] R-Ć+ A- R 0–H R—С—0—Н + Rate = k[RCOOH][R'OH][HA] k4 0–H R-ó+ A- Group 2 Rate = k[RCOOR']/{[RCOOH][R'OH]} H Rate = k[R'OH] 0–H Rate = k[RCOOH] k5 R- C-0–R' R-C-0–H + H,о + НА R-o+ A- Group 3 Step 2 or Step 3 O Step 1 or Step 2 Step 1 Step 3 Step 2 Step 1