Find the following answers to questions 1-3 from the information in the picture provided please. 1. Initial concentration of iodine in reaction (mM)2. Initial concentration of hydrogen peroxide in reaction (mM)3. Initial rate (mM/s) CS IODINE CLOCK REACTION|Lab DataConcentrationConcentration of iodide solution (mm)Concentration of thiosulfate solution (mm)Concentration of hydrogen peroxide solution (mm)Temperature of iodide solution (°C)Volume of iodide solution (1) used (mL)Volume of thiosulfate solution (S203²-) used (ml)Volume of DI water used (mL)Volume of hydrogen peroxide solution (H₂O₂) used (mL)Time (s)ObservationsInitial concentration of iodide in reaction (mm)Initial concentration of thiosulfate in reaction (mm)Initial concentration of hydrogen peroxide in reaction (mm)Initial Rate (mm/s)TemperatureTrial 173.931.5145.525.010.01.02.57.528.9Liquid turned darkblue at 28.9seconds1.57.0Trial 273.931.5145.5Trial 373.931.5145.5- XU

The objective of the question is to calculateThe initial concentration of .The initial concentration…

S IODINE CLOCK REACTION A Lab Data F Concentration Concentration of iodide solution (mm) Concentration of thiosulfate solution (mm) Concentration of hydrogen peroxide solution (mm) Temperature of iodide solution (°C) Volume of iodide solution (I) used (mL) Volume of thiosulfate solution (S₂03²-) used (mL) Volume of DI water used (mL) Volume of hydrogen peroxide solution (H₂02) used (mL) Time (s) Observations Initial concentration of iodide in reaction (mm) Initial concentration of thiosulfate in reaction (mm) Initial concentration of hydrogen peroxide in reaction (mm) Initial Rate (mm/s) Trial 1 73.9 31.5 145.5 25.0 10.0 1.0 2.5 7.5 28.9 Liquid turned dark blue at 28.9 seconds 1.5 7.0 Trial 2 73.9 31.5 145.5 Trial 3 73.9 31.5 145.5 -

S IODINE CLOCK REACTION A Lab Data F Concentration Concentration of iodide solution (mm) Concentration of thiosulfate solution (mm) Concentration of hydrogen peroxide solution (mm) Temperature of iodide solution (°C) Volume of iodide solution (I) used (mL) Volume of thiosulfate solution (S₂03²-) used (mL) Volume of DI water used (mL) Volume of hydrogen peroxide solution (H₂02) used (mL) Time (s) Observations Initial concentration of iodide in reaction (mm) Initial concentration of thiosulfate in reaction (mm) Initial concentration of hydrogen peroxide in reaction (mm) Initial Rate (mm/s) Trial 1 73.9 31.5 145.5 25.0 10.0 1.0 2.5 7.5 28.9 Liquid turned dark blue at 28.9 seconds 1.5 7.0 Trial 2 73.9 31.5 145.5 Trial 3 73.9 31.5 145.5 -

Chemistry In Focus

6th Edition

ISBN:9781305084476

Author:Tro, Nivaldo J., Neu, Don.

Publisher:Tro, Nivaldo J., Neu, Don.

Chapter11: The Air Around Us

Section: Chapter Questions

Problem 4SC

See similar textbooks

Similar questions

An inexperienced graduate student moved into a laboratory and began work. He needed some diethyl etherfor a reaction, so he opened an old, rusty 1-gallon can marked “ethyl ether” and found there was half a gallon left. To purifythe ether, the student set up a distillation apparatus, started a careful distillation, and went to the stockroom for the otherreagents he needed. While he was at the stockroom, the student heard a muffled “boom.” He quickly returned to his lab tofind a worker from another laboratory putting out a fire. Most of the distillation apparatus was embedded in the ceiling.(a) Explain what probably happened.(b) Explain how this near-disaster might have been prevented
Solid potassium sulfide is slowly added to 150 mL of a 0.277 M nickel(II) iodide solution until the concentration of sulfide ion is 0.0269 M. The percent of nickel ion remaining in solution is %. 20 Submit Answer $ 4 R F M 07 20 Retry Entire Group % 5 [Review Topics] [References] Use the References to access important values if needed for this question. T Cengage Learning Cengage Technical Support G ^ 6 8 more group attempts remaining D MacBook Pro Y H & 7 N U * 00 8 J I M 69 K O ) 0 < A L P A Previous Next Email Instructor { Save and Exit ~4 ? 1
Help Aluminum metal reacts with nitric acid to produce aluminum nitrate and hydroger gas, identify the palanced reaction that describes this process. Mutuble Choice A A HNÖ3-- AINO3- H2 Al + 3HNO3 – AKNO33 - H2 Al - 2HNO3 - AIINO3|2 - H2 2A1 - O INO, - 2AIINOg - 3H2 Al - HNO3 - AINO, +H
Module 8: H X 7087483#/7087483/16/2 % General Chemistry 4th Edition McQuarrie Rock Gallogly Question 25 of 35 - Module 7 Ho X [13] = x10 TOOLS Topic: Week 4 Discussion Resources C Give Up? The amount of I5 (aq) in a solution can be determined by titration with a solution containing a known concentration of S₂O3(aq) (thiosulfate ion). The determination is based on the net ionic equation 2S₂O3(aq) + 13(aq) →SO (aq) +31-(aq) Given that it requires 41.0 mL of 0.450 M Na₂S₂O3(aq) to titrate a 20.0 mL sample of I3 (aq), calculate the molarity of 15 (aq) in the solution. Hint University Science Books presented by Macmillan Learning M Question Source: McQuarrie, Rock, And Gallogly 4e-General Chemistry C C
balanced molecular equation (ME) write the balanced complete ionic equation (CIE) and write the balanced net ionic equation (NIE) Tin(II) chloride + potassium nitrate SnCl2(aq) KNO3(aq) Observations: No observable change; solution mixture is clear and colorless ME: CIE: NIE:
Name:Tashina B. 4-16-22 Period: 7 Conservation of Mass - Balance Equations Skeleton ** Success Criteria: I can determine that in a chemical reaction matter just changes forms, but the amounts of matter do not change. Directions: Place the number on the blank line for the coefficient that makes the following reactions balanced. 1. NaClO3- NaCl + 0₂ 2. (NH4)3PO4 + Pb3(PO4) 4+ NH4NO3 3. ZnS + Al₂S3 Ag₂S → Sn(NO₂)4+ KBr + C₂H₁7 + KOH + 5. 6. 7. 8. Pb(NO3)4 → AIP → Ag + Pt3N4 → Fe(OH)₂ O₂ → Co3(PO4)2 → Zn₂P₂ + S8 Sn, N4 + KOH + CO₂ + H₂O K₂PO4 + Pt(NO₂)4 FeBr3 Co(OH)2
> (1_101232) (2) el 25 April-1 May > MidExam-28-4-2021 ne Calendar Badges All courses What is the oxidation state of iron in K4FE(CN)6? O a. 2+ O b. 4+ O c. 6+ Od. 3+ 4 £5 . 6 T 7 v8 A9 R TY Y !U 10
The chemical reaction Fe[SCN]2⇋ Fe+2 +2SCN- a)is it endothermic or exothermic? b)What would happen if SCN- was decreased? c)What would happen if Fe+2 was increased?
gs Review View Help >T T< AaBbCcDd AaBbCcDd AaBbCC AABBCCC Aa 1 Normal 1 No Spac. Heading 1 Heading 2 Title Paragraph Styles When sodium sulfide reacts with cobalt (II) acetate in water, cobalt (II) sulfide and sodium acetate are produced. (a) Write the balanced (i) molecular; (ii) total ionic; and (iii) net ionic equations. Include phases. (b) If 4.00 mL of 0.250 mol/L sodium sulfide solution are reacted with 6.80 mL of 0.350 mol/L cobalt (II) acetate solution, what mass of precipitate is formed? Show all your work, including a complete dimensional analysis. (c) Assume the reaction proceeds to completion with 100% yield and that the excess reactant could not be recycled. What is the mass of wasted starting material? DELL
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
A student use solution of potassium hydroxide to titrate a solution of nitric acid. Which question is the student trying to answer? uch nitric acid solution is present? ow many moles of potassium hydroxide are present? O What is the concentration of potassium hydroxide? O What is the concentration of nitric acid? https://prodpcx-cdn-learnosityassessmentviewer.emssvc.connexus.com/index.html# Type here to search
TYPES OF REDOX REACTION No. Procedure Observation Balanced Chemical Equation Types of Redox Reaction 1 Mg ribbon + heat 2 Sodium bicarbonate + HCl 3a Aluminum foil + Hydrochloric acid 3b Iron + Copper (II) sulfate 4a hexane + heat 4b Kerosene + heat 5 Hydrogen peroxide + vinegar