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? At 25°C, the reaction, I(aq) + OCI (aq) → Ol(aq) + Cl(aq), has the following rate law:Rate (0.827 L mol¹ s¹) [I][OC].Calculate the rate of the reaction when:(a)[I] 0.0146 M and [OCI] = 0.0454 M: Rate = imol L-1 s-1(b)[I]=0.140 M and [OCI] = 0.0485 M: Rate=mol L-1 s-1

Answered: Image /qna-images/answer/ee3eedc2-8022-47fd-9791-c206452cbd65.jpg

At 25°C, the reaction, I(aq) + OCI (aq) → Ol(aq) + Cl(aq), has the following rate law: Rate (0.827 L mol¹ s¹) [I][OC]. Calculate the rate of the reaction when: (a) [I] 0.0146 M and [OCI] = 0.0454 M: Rate = i mol L-1 s-1 (b) [I]=0.140 M and [OCI] = 0.0485 M: Rate= mol L-1 s-1

At 25°C, the reaction, I(aq) + OCI (aq) → Ol(aq) + Cl(aq), has the following rate law: Rate (0.827 L mol¹ s¹) [I][OC]. Calculate the rate of the reaction when: (a) [I] 0.0146 M and [OCI] = 0.0454 M: Rate = i mol L-1 s-1 (b) [I]=0.140 M and [OCI] = 0.0485 M: Rate= mol L-1 s-1

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

Related questions

Q: Please don't provide handwritten solution

A: The objective of the question is to calculate the concentration of reducible iodine.

Q: A 1.000-g sample containing K2C2O4 (166.21 g/mol) is titrated with 40.00 mL of .0200 M KMNO4 in:…

A: Given 1g sample has K2C2O4 titrated with potassium permanganate, we have to find normality of…

Q: What is going on in the hexane layer at the end of a Group I Anion experiment? On a qualitative…

A: The given experiment is to identify the and anions.

Q: 5. Based on your reading about qualitative analysis and your knowledge of the solu rules, consider…

Q: A)Write the basic equilibrium equation for HONH₂ B)Write the acidic ionization equation for H₂SO₄…

A: A) When NH2OH dissolved in water, it dissociates into ions. NH2OH(aq) + H2O(l)⇌NH3OH+(aq) + OH-(aq)…

Q: 2. 15.0 mL HNO3 was titrated to equivalence with 60.0 mL of 0.020 NAOH, What is the concentration of…

A: Given : Volume of HNO3 = 15.0 mL Molarity of NaOH = 0.020 M Volume of NaOH = 60.0 mL To…

Q: only need help with the average molarity of KMnO4 solution (M) it must be a number. Reaction…

Q: For a 1.0 x 10-4 M solution of HCIO(aq), arrange the species by their relative molar amounts in…

A: Given: Concentration of HClO = 1.0×10-4 M

Q: For a water sample with a bicarbonate ion concentration of 50 mg/L and a CO2 content of 30 mg/L: a)…

Q: MaVa-MbVb can be used for simple strong acid- strong base titration calculations. Suppose 125 mL of…

Q: 7) Give the reaction type for each of the following reactions. (2 points each) -> a. Pb(OH) 2 (s) →…

A: The reaction Pb(OH)2 (s) → PbO (s) + H2O is a decomposition reaction. In a decomposition reaction, a…

Q: A buffer solution made from hydrocyanic acid and potassium cyanide was titrated with hydrochloric…

A: A buffer solution maintains a constant pH upon addition of a small amount of acid or base. They are…

Q: A solution of HNO3HNO3 is standardized by reaction with pure sodium carbonate. 2H+ + Na2CO3⟶2Na+…

A: Given Data Volume = 28.30 ± 0.06 mL =0.02830± 0.0006 L 0.8450 ± 0.0009 g of Na2CO3, (FM 105.988 ±…

Q: We did a lab and have to answer the following question: What was the concentration of the NaOH…

A: The balanced chemical equation for the reaction of NaOH and KHP is given below.

Q: Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant…

A: Answer: Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: Sodium error encountered in using a pH meter causes a/an decrease in the pH reading of a solution…

A: This statement is true. Things to understand : pH Sodium Error and the Effect on ph meter reading…

Q: Part A Calculate the molar concentration of OH ions in a 0.520 M solution of hypobromite ion (BrO;…

A: We know , PH = [OH-] , PH + pOH = 14

Q: It is desired to prepare 900mL of 0.125 normal Ca(OH)2 for use in the reaction: 2HCl + Ca(OH)2 =…

A: The given data contains, Volume = 900 ml = 0.9 LNormality =0.125 N

Q: Jessica made 300 mL of primary standard using 2.35 g of sodium carbonate. She then conducted a…

A: Given - Mass of primary standard, sodium carbonate = 2.35 g and its volume is = 300…

Q: in text form with proper workings and explanation for each and every part and steps with concept and…

Q: H₂O M solution of NH₂CIO (aq), arrange the species by their relative molar amounts in solution. H₂O*…

A: Molar concentration of NH4ClO4 = 1.0 x 10-2 M = 0.01 M When it is ionized, it is dissociated to…

Q: fill in the blanks please a. In the laboratory, a general chemistry student measured the pH of a…

A: Acid dissociation constant Kb is utilized to determine the basic nature of a solution. It refers to…

Q: A O CHEMICAL REACTIONS Determining the molar mass of an acid by titration…

A: Here we are required to find the molar mass of the monoprotic acid.

Q: If 0.025 moles of hypobromous acid (HOBr, a weak acid) is dissolved in 1 liter of water (HOBr ↔ H+ +…

A: The objective of the question is to determine the correct mole balance equation for the dissociation…

Q: A 2.00 L graduated cylinder contains 1.40 L of buffer solution. The density of the buffer solution…

Q: A 5.00 ml sample of vinegar was titrated with 0.08751 M NAOH. The sample requires 22.31 mL of NaOH…

Q: II. Your calcium carbonate antacid tablet weighed 1.50 g. You added 25.00 mL of a 1.00 M solution of…

A: " Since you have posted a question with multiple sub-parts as per company policy we will solve first…

Q: When the following equation is balanced properly under acidic conditions, what are the coefficients…

Q: As you are studying for finals, you calculate the concentration of caffeine in an energy drink and…

A: Given: Mass of caffeine = 257 mg = 0.257 g (Since 1 g =…

Q: bbhosted.cuny. ebapps/asessme assessment_id=_2032637_1&course_id= 201483... Remaining Time: 1 hour,…

Q: Calculate the mass, in grams, of potassium iodide that must be added to a 125-mL volumetric flask in…

Q: 3. Traces of heavy metals, such as Cu²* and Pb²*, in water bodies can be separated through…

A: To calculate the initial molar concentration of heavy metal ions present in the sample.

Q: 7. A student used acidified Fe²+ (aq) to standardize a solution of K₂Cr₂O, The data for the trial…

A: Here we are given the titration of Fe2+ vs K2Cr2O7. 25 ml of 0.3 M Fe2+ was used and the volume of…

Q: only need help with the average molarity of KMnO4 solution (M) it must be a number. The answer is…

Q: help please answer in text form with proper workings and explanation for each and every part and…

A: 1. Write the equilibrium constant expression (Ka):Ka = [H3O+][Ac-] / [HAc] 2. Plug in the known…

Q: Review I Consta Part A Explain the difference between a strong and weak electrolyte. Give an example…

A: Electrolyte :- A solution that contains ion is called an electrolyte solution. Electrolyte is…

Q: Be sure to answer all parts. The active agent in many hair bleaches is hydrogen peroxide. The amount…

Q: Find Moles NaOH required for titration HC2H302 NaOH -> H20NaC2H302 Volume of vinegar sample…

A: The given titration is an acid-base titration.

Question

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?

At 25°C, the reaction, I(aq) + OCI (aq) → Ol(aq) + Cl(aq), has the following rate law:
Rate (0.827 L mol¹ s¹) [I][OC].
Calculate the rate of the reaction when:
(a)
[I] 0.0146 M and [OCI] = 0.0454 M: Rate = i
mol L-1 s-1
(b)
[I]=0.140 M and [OCI] = 0.0485 M: Rate=
mol L-1 s-1

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH, CH, CO, H, pK, = 4.874). + log Answer Bank pH pK [A] [HA] Using the equation to calculate the quotient [A /[HA] at three different pH values. [A ] [HA] pH = 4.373 [A] pH = 4.874 [HA] [A] [HA] pH = 5.186
Suppose you perform an experiment tracking the formation of a product over time, resulting in the black points on the given plot. Product Concentration 0.4 0.35 0.3 0.25 0.2 0.15 0.1 0.05 0 0 A Select one: 5 B 10 The red line, A 15 Time (s) The green line, B The blue line, C The purple line, D 20 D Which tangent line represents the slope you should use to determine the initial rate of the reaction? 25 30
Hello, I'm going wrong somewhere in solving. Could you help me? Picture attached
A student is studying the reaction: 2 CrO4 + 2 H30 Cr207 + 3 H2O If CrO4 is yellow and Cr207 is orange, what colour would the reaction mixture turn if concentrated NaCrO4 was added to the reaction? Type your answer and submit X₂ X² Write your response here... Unanswered := 8 Explain your answer from question 7 Submit
None
In lab, you will be provided with a 1.8 M acetic acid solution (CH3COOH) and a 1.0 M NaOH solution. You want to make 100.0 mL of a 0.5 M acetic acid buffer at pH 5.00. What volume (mL) of the 1.8M acetic acid solution, NaOH solution, and deionized water should you combine? Show all work.
3. For the reaction below calculate the [F] and [Ba2] in solution in mo given a keq = 1.84 x 10-7 and a total volume of 500 mL. Place your answer on the line below. Give your answer to three significant figures and show your work. [F] (M): [Ba¹2] (M): BaF2 (s) Ba¹2 (aq) + 2F (aq)
Titrated with 0.3554 M NaOH True molarity of unknown: 0.5018 M Trial 1 Trial 2 trial3 The volume of acid added to flask (mL) 10.00 10.00 10.00 Initial buret reading (mL) 0.00 14.06 28.19 Final buret reading (mL) 14.06 28.19 42.30 Volume of base titrated into flask 14.06 14.13 14.11 calculated molarity of acetic acid in your unknown A) calculate the molarity of acetic acid in your unknown for each trial. b) choose the three trials that have molarities that agree within 1% of one another and use these three molarities to calculate average c)use the true molarity for your acetic acid solution from above. using the average molarity that you calculated above calculate the percent error for your unknown.
i need typing clear urjent
Use ICE table, solve Ka, and the pH based off table/Ka. Show all work, thank you!
Please answer Q1
I am doing a prelab and I need help with the questions. I want to make sure I did everything right. We are using the group 1 ions: Hg2+, Ag+, Pb2+