These questions are based on a reaction rate lab for my Chemistry homework. I attached my data values that I have already calculated. I think I am supposed to show more work for 4 and 5. I am genuinely confused on how to plot the graph too (6-7). Lastly, I am not sure if I got 8-10 correct? I think the rate law might be Rate = k [HCl] [Na2S2O3] but I am not sure if it needs an exponent or not? 1. Calculate the final concentration of hydrochloric acid and sodium thiosulfate in eachreaction. (M,V, = M2V2)[HCI] inExpt.Expt.1.0 M HCI0.30 MH20Final[NazS203]In Expt.Volume(mLadded)Na2S203(mLadded)(mLadded)(mL)1325 mL0.60.1221.51.55 mL1.50.1231225 mL0.20.124235 mL0.40.1821.51.55 mL0.40.096215 mL0.40.06Data Table 1 for Varying the Concentration of HCIExpt.Final [HCI]Final [NazS203]Time (s)Rate (1/s)10.60.12370.02701.50.12430.023230.20.12390.0256Data Table 2 for Varying the Concentration of Na2S203TrialFinal [HCI]Final [NazS203]Time (s)Rate (1/s)40.40.18340.029450.40.09620.01610.40.061310.00762. 4. Based on your data in Data Table 1, does the reaction rate depend on the HCl concentration? If so, how? What is the reac-tion order for HC1 It dependo an Na2 Sz03 only. The reaetion ordernowould be 1st order.y due to Data 1 showing HCl does notapuit recetion tint anificantly.5. Based on your data in Data Table 2, does the reaction rate depend on the Na,S,0, concentration? If so, how? What is thereaction order for Na,S,O,? It dpends on Nazsz03.→ beconed I2 reuetron tine amount.Itas afirst order reeetscn vate. HCI-zero orderr reaction.6. Plot a graph showing the reaction rate vs. [HCI] using the data from Data Table 1. What is the shape of the resulting plot?7. On the same graph, plot the reaction rate vs. [Na,S,O,] using the data from Data Table 2. What is the shape of the resultingplot?8. What is the overall order of the reaction? -→ averal reaetion roate = first ordr(1)1ot order reaction. for Naz Sz03. Zero order for HCl.%3D9. Write the rate law for this reaction.10. Based on the rate law you determined, what are the units on the rate constant, k?sec-!"

HCIS zeo order reaeticn. 6. Plot a graph showing the reaction rate vs. [HCI] using the data from Data Table 1. What is the shape of the resulting plot? 7. On the same graph, plot the reaction rate vs. [Na,S,0,] using the data from Data Table 2. What is the shape of the resulting plot? 8. What is the overall order of the reaction? overal reaetion rate = first ordur (1 order reaction.for NazSz03. Zero order for HCl. 9. Write the rate law for this reaction.

HCIS zeo order reaeticn. 6. Plot a graph showing the reaction rate vs. [HCI] using the data from Data Table 1. What is the shape of the resulting plot? 7. On the same graph, plot the reaction rate vs. [Na,S,0,] using the data from Data Table 2. What is the shape of the resulting plot? 8. What is the overall order of the reaction? overal reaetion rate = first ordur (1 order reaction.for NazSz03. Zero order for HCl. 9. Write the rate law for this reaction.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter9: Aqueous Solutions And Chemical Equilibria

Section: Chapter Questions

Problem 9.2QAP

See similar textbooks

Similar questions

Moles of NaOH at the equivalence point? Mass of H2C2O4·2H2O= 1.32191 g Volume of the H2C2O4·2H2O solution= 250.0 mL
In a sulfuric acid (H2SO4) - Sodium hydroxide (NaOH) acid-base titration, 17.3 mL of 0.126 M NaOH is needed to neutralize 25 mL of H2SO4 of unknown concentration. Find the molality of the H2SO4 solution, given that the neutralization reaction occurs is: H2SO4 (aq) + NaOH (aq) ----> Na2SO4 (aq) + H2O (l)
the percentage of KHP in an unknown sample was determined. Which of the following is NOT true. Aqueous NaOH should be standardized so concentration is accurately known. The moles of KHP can be determined at the endpoint, which is close to the equivalence point. Percentage of KHP, is equal to the mass of KHP found, divided by the mass of the unknown, multiplied by 100.
Consider a solution made by mixing 500.0 mL of 4.0M NH3 and 500.0mL of 0.40MAgNO3.Ag+ reacts with NH3, to form AgNH3+ and Ag(NH3)2+: Ag+(aq)+NH3(aq)AgNH3+(aq)+NH3(aq)⇌AgNH3+(aq)⇌Ag(NH3)2+(aq)K1=2.1×103K2=8.2×103 Determine the concentration of all species in solution. asap please.
Normality is same as Molarity for sodium hydroxide and normal = molar (for NaOH) Normality of sodium hydroxide = 0.10395N (normal) or Molarity of NaOH = 0.10395M (molar) Volume of NaOH consumed during the titration = 21.87 mL Mol wt of Naproxen = 230.26 g/mol Weight of Naproxen ds (i.e., sample) = 0.534g Calculate the % Purity (dried-basis) of Naproxen ds, given that the LOD results for Naproxen = 1.0% a 97.0 b 98.0 c 98.5 d 99.0 e 99.5 f none of the other answers.
How many mls of 1 M NaOH titront are needed to react with 5 mls of 0.1 KHT? (Use the ml*M/ coefficient= ml*m/coefficient formula to solve this problem)
At a particular temperature and pressure, the dissociation constant for water (Kw) is 3.9×10-15. What is the pOH of pure water under these conditions? Your answer must be entered to the hundredth decimal place.
16. Concentrated glacial acetic acid is 99.7% H3CCO2H by mass and has a density of 1.05 g/mL. What is the molar concentration of concentrated glacial acetic acid? Group of answer choices A. 1750 M B. 17.5 M C. 1.75 M
How many mL of 0.112M Pb(NO3)2 are needed to completely react with 25.0mL of 0.105M KI? Given: Pb(NO3)2 + 2KI -> PbI2 + 2KNO3.
A 3.00 mL aliquot of 0.001 M NaSCN is diluted to 25.0 mL with 0.1 M HNO3. How many moles of SCN- are present?
1. Calculate the moles of KHP you titrated for each trial. (KHP is KHC8H4O4). MW = 204.23 g/mol. Determine the number of moles of NaOH required to neutralizw the KHP. Use the mole-mole ratio provided inthe balanced equation. Place answers in data table 2(second picture format) 2. Calculate the volume, in mililiters, of NaOH used to neutralize the KHP. Convert to Liters. Place answers in data table 2. 3. Calculate the molarity of the NaOH solution in units of moles/liter. Place answers in data table 2.
A student prepared a 1:1 buffer, for which [HAc] = [Ac-] = 0.05182 M. Using their 1:1 buffer and a 0.10229 M HCl solution, the student prepared Solution C in Part 3 of the experimental procedure. Given this information, how many moles of Ac- were there in the student's Solution C after a reaction took place? Report your final answer, in moles, to 6 decimal places and only include the numerical value (no units). Solution C contains 20mL of buffer and 5mL of HCl.