Given the reaction below: 3 CIO (aq) → CIO3(aq) + 2 CI (aq) Which of the following is the CORRECT rate expression with respect to the reactant, CIO? 2 ACROT rate= 3 rate - 3 AGIOT 2 Al rate = 3 AGIOT] At 1 A|CO| 3 AL O O rate

Given the reaction below: 3 CIO (aq) → CIO3(aq) + 2 CI (aq) Which of the following is the CORRECT rate expression with respect to the reactant, CIO? 2 ACROT rate= 3 rate - 3 AGIOT 2 Al rate = 3 AGIOT] At 1 A|CO| 3 AL O O 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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2. Consider the reaction that occurs when a CIO2 solution and a solution containing hydroxide ions (OH) are mixed at 0°C, shown in the following equation. 2CIO2(aq) + 2OH (aq) → Cl03° (aq) + CIO2° (aq) + H2O (1) When solutions containing CIO2 and OH- in various concentrations were mixed at 0 oC, the following rate data were obtained: Determination Initial concentration Initial concentration of Initial rate for formation number of ClO2, mol/L OH", mol/L of CIO3¯ mol/Ls 1.25x10-2 1.30x10-3 2.33x10-4 2.50x10-2 1.30x10-3 9.34x104 3 2.50x10-2 2.60x103 1.87x10-3 a) Use the method of initial rates to find the order of the reaction with respect to CIO2 and with respect to OH. Write the rate equation for the reaction of CIO2 and OH´ at 0°C. b) Calculate the rate constant, k, for the reaction of clO2 and OH at 0°C. c) Calculate the reaction rate for the reaction CIO2 and OH at 0°C when the initial ClO2 and OH concentrations are 8.25x10-3 mol/L and 5.35x 10-² mol/L, respectively. 1.
Correct Expressed in terms of x, y, and z, the rate law is as follows: The iodate ion, IO3¯, is reduced by sulfite, SO32", according to the following net ionic equation: rate = kæyz By substituting the actual species from the reaction, the expression becomes I03 (aq) + 3S03²- (aq)→I¯(aq) + 3SO,²-(aq) k[IO3 ][SO3²-][H*] rate = Part B By what factor will the rate of the reaction change if the pH changes from 6.50 to 2.00? Express your answer numerically using two significant figures. • View Available Hint(s) 3.2 • 10-5 Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining Because it is less than one, your answer implies that the rate decreases. However, lowering the pH raises the hydrogen ion concentration. Part C The reaction is pH dependent even though the H+ ion does not appear in the overall reaction. Which of the following explains this observation? Check all that apply. • View Available Hint(s) O H+ serves as a catalyst in the reaction. The exponent of H+ in the rate…
A student suspects that the nitrate ion (NO3−), rather than the Cu2+ ion, is the active species in the Cu(NO3)2 catalyst. He devises a second experiment to test his hypothesis, using KNO3 as a potential catalyst. If the student's hypothesis is correct, what should he observe when KNO3 is added to the reaction? Any changes are observed relative to an identical un-catalyzed reaction. a. The rate of the reaction will decrease b. The rate of the reaction will increase c. There will be no change in the rate of the reaction
Please answer all parts.
In the reaction 2 N2O5 → 4 NO2 + O2 given that the rate law is v = k[N2O5] where v is the reaction rate or reaction velocity, calculate the rate of formation of NO2 if the instantaneous rate of reaction is 1.6 x 10−6 mol L−1 s−1. Insert answers in the form x.xE±x and include units
6) For the reaction 3A + 2B2C + D + E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected: Rate (M/s) 1.9 x 108 [A] (M) [B] (M) 1.0 x 10¹2 1.0 x 10¹1 9.5 x 108 5.0 x 10¹2 1.0 x 1011 3 5.7 x 108 1.0 x 10¹2 3.0 x 10¹1 a) Write the rate law for this reaction. rate=[A]*[B]Y 3 3.0 x 10" 1.0 x10¹2 y = ²/ 5.0×10 1.0x1010 X = = 1 1.0x10" 1.0 ×1010 5 3=1 b) What is the overall order of the reaction? c) Calculate the rate law constant, k (including units). x = = 1.0x10" 1.0 x 10" 1 lom C²
Give answer to all parts
Peroxynitric acid (HOONO2) is an unstable molecule that decomposes to nitric acid and oxygen: 2HOONO2(aq) → 2HNO3(aq) + O2(g)When the concentration of peroxynitic acid is graphed against time, the resulting plot is curved, but if the logarithm of this concentration is plotted, we instead get a straight line. Based on this, which statement is true? a) This decay is a second order in peroxynitric acid. b) The slope of the straight-line graph is the rate constant. c) One needs the concentration of peroxynitric acid to calculate its half-life. d) The rate law appears to be of the form -Δ[HOONO2]/Δt = k[HOONO2].
For the reaction aA + bB Products, the rate law for the reaction is given by Rate = k[B]. Choose the correct answer. %3!
2. Suggest method(s) that can be used to measure the rate of reaction of the following reactions. Explain your choices. (There may be more than one method in each of the following reaction.) 5H,O,(aq) + 2MNO, (aq) + 6H¨(aq) → 2Mn²*(aq) + 8H2O(1) + 502(g)
Consider the reaction 5Br (aq) + BrO, (aq) + 6H+ (aq)→3B12 (aq) + 3H20(1) The average rate of consumption of Br is 1.36x104 M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval? Express your answer with the appropriate units. • View Available Hint(s) HẢ |] ? Rate of formation of Br2 Value Units %3D
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