The lodate 103 , Is reduced by sulmte, SO3 according to the following net ionic equation: rate = kryz By substituting the actual species from the reaction, the expression becomes IO3 (aq) + 3SO3²-(aq)→I¬(aq)+3SSO,²-(aq) rate = k[IO3 ][SO3²-][H*] 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-s 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. O The exponent of H*] in the rate law is zero. O H+ enters the reaction mechanism after the rate-determining step. O H+ is an intermediate in the reaction mechanism. Submit

The lodate 103 , Is reduced by sulmte, SO3 according to the following net ionic equation: rate = kryz By substituting the actual species from the reaction, the expression becomes IO3 (aq) + 3SO3²-(aq)→I¬(aq)+3SSO,²-(aq) rate = k[IO3 ][SO3²-][H] 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-s 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. O The exponent of H] in the rate law is zero. O H+ enters the reaction mechanism after the rate-determining step. O H+ is an intermediate in the reaction mechanism. Submit

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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R=K [A] [B] ----; 2. The initial rate of the reaction: BrO3(aq) + 5 Br (aq) + 8 H*(aq) Has been measured at the reactant concentrations shown (in mol/L): Trial [BrO3] [Br] [H*] 1 0.10 0.10 0.10 2 0.20 0.10 0.10 3 0.10 0.20 0.10 4 0.10 0.10 0.20 A) Determine the rate law equation including the k value. Determine the order of reaction for BrO3, Br, and H* Rate law 3 Br₂(l) + H₂O(l) Initial rate (mol/Ls) 8.0 x 104 1.6 x 10³ 1.6 x 10°³ 3.2 x 10'³
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The initial rate of the reaction is determined for different initial conditions, with the results listed in the table. (a) What is the overall reaction order? (b) What is the value of the rate constant, k
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See attached image for question A.) What is the order of the reaction in A? B.) What is the rate of reaction when the initial concentrations are [A]= 0 M and [B]= 4.4x 10-2M?
The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: со + Clz → COCI2 Initial Rate, Ms-1 Experiment [CO]o, M [CIz]o, M 2.45 0.399 1.43x10-28 2 2.45 0.798 |2.85х10-28 3 4.90 0.399 2.85x10-28 4 4.90 0.798 5.71x10-28 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]^ , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is M-1s-1.
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The rate of a certain reaction is given by the following rate law: rate =k N, O, Use this information to answer the questions below. olo What is the reaction order in N,? |x10 18 Ar What is the reaction order in 03? What is overall reaction order? At a certain concentration of N, and 03, the initial rate of reaction is 0.780 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 5.0 x 103M/s when [N2] = 1.1 M and [03] = 1.1 M. Calculate the value of - 3 -1 k = |M •S the rate constant. Round your answer to 2 significant digits.
just need standard error for K
I completed the problem but for some reason, my answer is still wrong. for part a I got 5.48 x 10^-5 and for part b I got 5.61x10^-4. I substituted the concentrations in the equation but hey still seem to be wrong can someone explain?
The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCII → OI¯ + Cl¯ This rapid reaction gives the following rate data: |[OCI¯] (M) [I¯] (M) Initial Rate (M/s) 1.36 × 10-4 1.5 × 10- -3 3.0 × 10-³ 1.5 x 10- -3 1.5 x 10 -3 1.5 × 10-³ 3.0 × 10-³ 2.72 × 10-4 2.72 × 10-4 Calculate the rate constant with proper units. Express the rate constant to two significant figures. Indicate the multiplication of units, as necessary, explicitly either with a multiplication dot or a dash (e.g. ft * lb or ft-lb). k Submit Part C HÅ Value Request Answer Units ? Calculate the rate when [OC] = 2.3 × 10-³ and [I¯] = 6.0 × 10-4 Express the rate in molarity per second to two significant figures.
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