The iodide ion reacts with hypochlorite ion (theactive ingredient in chlorine bleaches) in thefollowing way:OCII → OI¯ + Cl¯This rapid reaction gives the following rate data:|[OCI¯] (M) [I¯] (M)Initial Rate (M/s)1.36 × 10-41.5 × 10--33.0 × 10-³1.5 x 10--31.5 x 10-31.5 × 10-³3.0 × 10-³2.72 × 10-42.72 × 10-4Calculate the rate constant with proper units.Express the rate constant to two significant figures. Indicate themultiplication of units, as necessary, explicitly either with a multiplicationdot or a dash (e.g. ft * lb or ft-lb).kSubmitPart CHÅValueRequest AnswerUnits?Calculate the rate when [OC] = 2.3 × 10-³ and [I¯] = 6.0 × 10-4Express the rate in molarity per second to two significant figures.

Answered: Image /qna-images/answer/fbeda319-04de-4f0e-89b2-4d08587032e4.jpg

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) 1.5 × 10-³ 1.5 × 10-³ 1.36 × 10-4 3.0 x 10-3 1.5 x 10-3 2.72 × 10-4 1.5 × 10-³ 3.0 x 10-3 2.72 × 10-4 with proper 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 O μÅ Value Request Answer Units ? Calculate the rate when [OCI] = 2.3 × 10-³ and [I] = 6.0 × 10-4. Express the rate in molarity per second to two significant figures.

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) 1.5 × 10-³ 1.5 × 10-³ 1.36 × 10-4 3.0 x 10-3 1.5 x 10-3 2.72 × 10-4 1.5 × 10-³ 3.0 x 10-3 2.72 × 10-4 with proper 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 O μÅ Value Request Answer Units ? Calculate the rate when [OCI] = 2.3 × 10-³ and [I] = 6.0 × 10-4. Express the rate in molarity per second to two significant figures.

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...

See similar textbooks

Similar questions

Using the information in the table, the value of the rate constant for the reaction A(g) + 3 B(g) → C(g) + 2 D(g) is
Suppose you are studying the kinetics of the reaction between nitrogen monoxide and hydrogen gas. You perform the reaction multiple times with different starting concentrations and measure the initial rate for each, resulting in this table. Experiment [NO] (M) [H2] (M) Initial Rate (M/s) 1 0.0050 0.0020 1.25 x 10–5 2 0.010 0.0020 5.00 x 10–5 3 0.0050 0.0040 2.50 x 10–5 Based on the data, choose the correct exponents to complete the rate law. rate=k[NO]x[H2]y x=? y=?
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…
Complete the following table for the first order reaction: A → product [A] k (min1) Rate (mol/L min) 0.200 2.0 x 103 (c) (b) 0.0372 0.035 6.82 (a) 7.98 x 103 (a) (b) (c)
The reaction 2 NO (g) + O2 (g) → 2 NO2 (g) occurs when automobile exhaust releases NO into the atmosphere. Use the following data to determine the order with respect to NO for this reaction. Trial [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.012 0.020 1.02 x 10-4 2 0.024 0.020 4.08 x 10-4 3 0.024 0.040 8.16 x 10-4 Enter the answer as a single digit, not the word.
- 1 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0020 M·s 2 HI (g) → H, (g) + I, (g) Suppose a 4.0 L flask is charged under these conditions with 150. mmol of hydrogen iodide. How much is left 5.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T
Given the following data, determine the rate constant of the reaction 2NO(g) + Cl2(g) –→ 2NOCI(g) Experiment [NO] (M) |Ck] (M) Rate (M/s) 0.0300 0.0100 3.4 x 104 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 104
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0022 M⚫s 1: 2 HI (g) →H₂ (g) +12(g) Suppose a 4.0 L flask is charged under these conditions with 250. mmol of hydrogen iodide. How much is left 7.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. X x10
The chemistry of smog formation includes NO3 as an intermediate in several reactions. If Δ[NO3] / Δt is –21.58×104 mM/min in the following reaction, what is the rate of appearance of NO2? NO3(g)+NO(g)---->2NO2(g) Δ[NO2]/Δt= mM/min What is the rate of change in [NO2] in the following reaction if Δ[NO3] / Δt is –22.56×10–1 mM/min? 2NO3(g)---->2NO2(g)+O2(g) Δ[NO2]/Δt= mM/min
"yonsanh Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. Reaction Molecularity Rate expression (a) NO2+NO2–→ 2 NO + 02 rate = (b) 0+O2+M →03+M rate = (c) NO,Cl–NO,+Cl rate =