The reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution OCI+I → OI+ CIT is first order in OCI and first order in I. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 8.58 x 10¹ M¹s¹. Using this value for the rate constant, the rate of the reaction when [OCI] = 6.80 x 10-³ M and [I] = 5.49 x 10-³ M would be M/s.

The reaction of hypochlorite ion with iodide ion in 1 M aqueous hydroxide solution OCI+I → OI+ CIT is first order in OCI and first order in I. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 8.58 x 10¹ M¹s¹. Using this value for the rate constant, the rate of the reaction when [OCI] = 6.80 x 10-³ M and [I] = 5.49 x 10-³ M would be M/s.

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

Solve all three parts otherwise I will downvote...
Be sure to answer all parts. The reaction of peroxydisulfate ion ( S,03-) with iodide ion (I) is S,03 (aq) + 31 (aq) → 2So,? (aq) + I3 (aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S,Og²](M) [I](M) Initial Rate [M/s] 1 0.0500 0.0840 7.60 x 104 2 0.0500 0.0420 3.80 x 10-4 3 0.1000 0.0420 7.60 x 104 (a) Which of the following equations represents the rate law for this reaction? A. rate = k[S,Og²0 B. rate = k[S,Og U C. rate = k[S,Og²O D. rate = k[S,O3 O A O B O со D (b) What is the rate constant for the reaction? k = M's
The first-order reaction, SO,Cl2 - SO2 + Cl2, has a rate constant equal to 2.20 x 10-5s1 at 593 K. What concentration of SO,Cl2 will remain after 25 minutes if the initial [SO,Cl2] is 0.450M? Enter your answer to 2 significant figures. Do not include the units, M.
The reaction for the formation of phosgene from carbon monoxide and chlorine Co + Cl,COC1, is first order in CO and first order in Cl,. Complete the rate law for this reaction in the box below. Use the form k[A]"B]"... , where '1' is understood for m, n. (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 1.85×10-23 M's1. Using this value for the rate constant, the rate of the reaction when [CO] = 0.877 M and [Cl] = 0.119 |Ms!. M would be
The reaction of UO," with hydrogen ion in aqueous solution 2 UO,* + 4 H* U4+ + UO,+ + 2 H,O is second order in UO,* and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A]™[B]"... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate =
D Other Bookmarks [References) Use the References to access important values if needed for this question. The reaction of nitrogen dioxide with fluorine 2 NO2 + F22 NO2F is first order in NO2 and first order in F2. Complete the rate law for this reaction in the box below. Use the form k[A]m[B]"..., where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 1.51x10-4 M-15-1 Using this value for the rate constant, the rate of the reaction when [NO2) = 1.95 M and [F2] = 2.97 M would be Ms-1, Submit Answer Try Another Wersion 2 item attempts remaining 7:15 PM 5/5/2022 SONY WEB K DISPLAY OFF One Touch Web Access Without Booting Up Delete F6 Num Lk Ser Lk Prt Sc Sys Ra Insert Pause F4 F7 BIG F12 F5 F8 F9 F10 F11 Break 1& Backspace - Home 6.
The reaction for the formation of phosgene from carbon monoxide and chlorine Co + Cl, → COC, is first order in CO and second order overall. Complete the rate law for this reaction in the box below. Use the form k[A]"B".. , where '1' is understood for m, n .. (don't enter 1) and concentrations taken to the zero power do not appear. Rate =
The reaction for the formation of phosgene from carbon monoxide and chlorine co + Ch → COCH is first order in CO and second order overall. Complete the rate law for this reaction in the box below. Use the form k[A]"B]"... , where '1' is understood for m, n .. (don't enter 1) and concentrations taken to the zero power do not appear. Rate =
The reaction of nitrogen monoxide with ozone at 25 °C NO + O3 NO2 + 02 is first order in NO and first order in 02. Complete the rate law for this reaction in the box below. Use the form k[A]"[B]"... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 111 M-ls1. Using this value for the rate constant, the rate of the reaction when [NO] = 0.117 M and [O3] = Ms 4.59x10-2 M would be
The reduction of nitric oxide with hydrogen 2NO+2H₂ → N₂ + 2H₂O is second order in NO and first order in H₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 0.0608 M-s¹, when [NO] = 0.498 M and [H₂] = 0.137 M. From this experiment, the rate constant is M-². s-¹.
Please don't provide handwritten solution....
The gas phase reaction of hydrogen with iodine H₂+I2 → 2HI is first order in H₂ and first order in I2. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 2.03 x 10-18 M¹s¹. Using this value for the rate constant, the rate of the reaction when [H₂] = 0.0356 M and [1₂] = 0.0123 M would be M/s.