The attached image shows the different amounts and concentrations for an iodide clock experiment, showing the effects of persulfate and iodide concentrations on reaction rate. How do I fill up this table? Please provide a general formula/solution for solving for the Molarity portion.
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The attached image shows the different amounts and concentrations for an iodide clock experiment, showing the effects of persulfate and iodide concentrations on reaction rate.
How do I fill up this table? Please provide a general formula/solution for solving for the Molarity portion.
Runs | [S2O8 2-], M | [I–], M | [S2O3 2-], M | Reaction time,s | Rate, M/s |
1 | 49.10 | ||||
2a | 106.10 | ||||
3 | 197.44 | ||||
4 | 69.20 | ||||
5 | 53.05 |
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Solved in 4 steps
- Reaction of interest : S2O82-(aq) + 3I- (aq)→ 2SO42-(aq) + I3-(aq). rate= k[S2O82-]1[I-]1.The formation of products in a gas-phase rxn is affected by A. Amount of reacting molecules B. All C. Number of Collisions D. Orientation of moleculesThe concentration of CH3NC was measured at a constant time interval of every 10 seconds over a 5.00 minute period for the isomerization of acetonitrile. CH3CN(g) --> CH3CN(g) The plot of ln[CH3NC] versus time in seconds produced the linear regression equation: y= -6.3x10-3(x) - 1.366 How much time does it take to reach 50% of the initial concentraion for this reaction? a.) 217 s b.) 150 s c.) 20.2 s d.) 110 s
- 1. The decomposition of aqueous sucrose to form the isomers glucose and fructose is a common organic reaction, which requires a strong catalyst: C12H22O11(aq) + H2O(l) → 2C6H12O6(aq). The following data were collected during the process: Time (min) [C12H22O11] (mol/L) 0 0.316 39 0.274 80 0.238 140 0.190 210 0.146 (a)If we performed a new trial with an initial concentration of sucrose of 0.400 mol/L, what concentration would remain after 4.0 h has passed? 2. Methyl isomerizes to acetonitrile, CH3NC(g) → CH3CN(g) at 215°C. The following data were collected during the process: Time (sec) [CH3NC] (mol/L) 2000 0.0110 5000 0.0059 8000 0.0031 12000 0.0014 15000 0.0007 2. (a)Assuming the process continues, what concentration of methyl isonitrile would we expect after 5.00 h?Consider the following reaction and the data provided.2 HgCl2(aq) + C2O4 2-(aq) ----> 2 Cl-(aq) + 2 CO2(g) + Hg2Cl2(s) Exp# [HgCl2] (M) [C2O42-] (M) Rate (M/s)1 0.164 0.15 3.2 x 10-52 0.164 0.45 2.9 x 10-43 0.082 0.45 1.4 x 10-44 0.246 0.15 4.8 x 10-5 What is the rate law? a) r = k[HgCl2] [C2O42-]2 b) r = k[HgCl2]2 [C2O42-]c) r = k[HgCl2] [C2O42-] d) r = k[HgCl2] [C2O42-]3Calculate the value of ΔrG for this reaction at 25 ∘C when the concentration of lead ions is 58 μM and the concentration of chloride ions is 26 μM. Given: Keq is 1.6x10-5 at 25∘C. PbCl2(s)↽−−⇀Pb2+(aq)+2Cl−(aq)
- For the following reaction 6 experiments have been run and the data collected is in the following table: 2 MnO4-(aq) + 5 H2C2O4 (aq) + 6 H+ (aq) ---> 2 Mn2+ (aq) + 10 CO2 (g) + 8 H2O (l) Experiment [MnO4-], M [H2C2O4], M [H+], M Rate, M/s 1 0.2410 0.3470 0.2690 0.1147 2 0.3260 0.6210 0.2270 0.2776 3 0.5630 0.5740 0.7420 0.4431 4 0.2410 0.3470 0.3840 0.1147 5 0.4140 0.5740 0.5610 0.3258 6 0.3260 0.4930 0.4910 0.2203 a) Find the order of the reaction with respect to H+. _______________ b) Find the order of the reaction with respect to MnO4-. ______________ c) Find the order of the reaction with respect to H2C2O4. _____________ d) What is the overall order of the reaction? ________________________UCI Chemistry researchers, Prof. F. Sherwood Rowland and Dr. Mario Molina werefirst to discovered in 1973 that chlorofluorocarbons (CFCs) were depleting the Earth’sozone layer when released into the atmosphere. Once they reach the stratosphere, Clis released from the CFCs molecules by interaction with UV light. Free Cl atoms areable to react with ozone in a catalytic cycle that converts O3into the more stable O2.It is estimated that a single Cl atom is able to react with∼100000 O3molecules.Although CFCs production was banned in 1996, there are still a substantial numberof motor vehicle air conditioners (MVACs) that use CFC-12 (CF2Cl2) as refrigerant.The average CFC-12 emission rate from operating MVACs has been estimated tobe 59.5 mg per hour per vehicle (Zhang et al.Environ. Sci. Technol. Lett.2017).How much chlorine, in kg, is added to the atmosphere in a year due to 100 millionMVACs using CFC-12 as refrigerant?For the following balanced equation, what is the rate of reaction with respect to [NH3]. N2 (g) + 3H2(g) →→ 2NH3 (g) A. ????=−2Δ[??3]Δ?Rate=−2Δ[NH3]Δt B. ????=−Δ[??3]2Δ?Rate=−Δ[NH3]2Δt C. ????=+3Δ[?2]Δ?Rate=+3Δ[H2]Δt D. ????=+Δ[??3]3Δ?Rate=+Δ[NH3]3Δt E. there is not enough information to answer the question
- Find the rate law constant and the order of the reaction a and b K[H2O]a[I-]b Concentrations: Starch 0.01 mol/L Buffer 0.5 mol/L Thiosulfate 0.02 mol/L Kl 0.25 mol/L H2O2 0.12 mol/L New concentrations after dilutions Reaction # V S2O3 (ml) V Kl (ml) V H2O2 (ml) Final volume (ml) S2O3 final M (mol/L) Kl final M (mol/L H2O2 final M (mol/L) t initial (s) t final (s) Rate S2O3 Rate of the reaction Log of rates Log of I Log of H2O2 1 5 6 5 100 0.001 0.015 0.006 81 718 7.85E-07 7.85E-07 -6.105169428 -1.823908741 -2.22184875 2 5 6 10 100 0.001 0.015 0.012 241 572 1.51E-06 1.51E-06 -5.820857989…If you have 100 gm of PET to be recycled with (EG/PET) molar ratio, 6, find the volume of Ethylene Glycol and the number of grams of catalyst that have to be used. First, take data: PET molecular mass is 192 g/mole based on monomer, and for EG 62.07 g/mole and its density (1.113 gm/cm3), the weight % of .Nano-Catalyst is 1 % base on PETFor the reaction 2N2O5(g) → 4NO2(g) + O2(g), the following data were collected. t (minutes) [N2O5] (mol/L) 0 1.24 × 10–2 10. 0.92 × 10–2 20. 0.68 × 10–2 30. 0.50 × 10–2 40. 0.37 × 10–2 50. 0.28 × 10–2 70. 0.15 × 10–2 The concentration of O2 at t = 10. min is Question 16 options: A) 0.32 × 10–2 mol/L B) 2.0 × 10–4 mol/L C) 0.64 × 10–2 mol/L D) 0.16 × 10–2 mol/L E) none of these