In the synthesis of hydrocarbons, the carbon source is carbon dioxide. Although the CO2 concentra?on in the atmosphere raises at a drama?c speed, point sources are probably the easier sources for a PtX process. Iden?fy 3 possible point sources, explain why CO2 is formed and what challenges each of the three CO2 streams presents
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In the synthesis of hydrocarbons, the carbon source is carbon dioxide. Although the CO2 concentra?on in the atmosphere raises at a drama?c speed, point sources are probably the easier sources for a PtX process. Iden?fy 3 possible point sources, explain why CO2 is formed and what challenges each of the three CO2 streams presents
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- Reaction Conc, Na,d O3| Cune. HCI 4Als. | AIme (3) Rabe I1.3085840 0.10M •30M 0.4563/64 |0.028 F0913 15 M 12267196 | 0,01870913 30M 1.5360817 0.300349 2 65.56796607 5. 11431671 O.10 M 3 0.050 M 4 0.025 M 0:30M 1.54866|1 1.007568 1,358380874 4. Use experimental data and the rate law to calculate a rate constant for each reaction 1, 2, 3, 4. How do the rate constants compare? Should they be the same or different? Discuss in your conclusions. Report the average value of your calculations. Be sure to include units in your rate constant. -1-4 -2:5 Rate= k [ Naz s03] [Hc1]|The Kc for CO(g) + 3H,(g) = CH,(g) + H2O(g) is 9.17 x 10-2. If a 3.5L vessel is set up with .o155 mol CO, 3.50 x 10-3 mol H2, .0100 mol CH4, and 7.60 x 10-4 mol H2O, what is the reaction quotient Qc? In which direction will this reaction proceed to reach equilibrium?3. In acidsolution, chlorate(V) ions, CIO; slowly oxidize chloride ions to chlorine. The following kinetic data are obtained at 25 °C. [CH)/ M Initialrate / Ms' 10 x 105 4.0 x 10 [CIO,1/M [H'1/M 0.20 Experiment 0.08 0.15 2 3 0.08 0.15 0.40 0.15 0.30 8.0 x 105 2.0 x 10 0.16 0.40 0.08 0.20 a. Write the halfequation for the oxidation of chloride ion to chlorine. b. Write the balanced equation for this reaction. Given the half equation for reduction is: 2CIO, + 10 e + 12H → C, + H20 c. Determine the order of the reaction with respect to each rea cta nt.
- 9-00 AM 21:SP-CHM- 22-061 OWLV2 | Online teachi G the organic moleculer [Review Topics] [References] Use the References to access important values if needed for this question. For the gas phase decomposition of hydrogen peroxide at 400 °C 2 H,O22 H,0+02 the following data have been obtained: 4.62x10-2 23.0 [H,O2], M 0.149 2.73x10-2 1.89x10-2 time, s 46.0 69.0 The average rate of disappearance of H2O, over the time period from t= 23.0 s to t= 46.0 s is Msl.Calcule el potencial estándar de la media reacción: HgS(s) + 2 H* (aq) + 2 e --> Hg() + H2S(g) si para la celda a continuación: Cd [Cd2*(1 M) || HgS(s) H* (1 M)| Hg() | H2S(1 atm)| Pt E°celda= -0.317 V y E° (Cd2+/Cd)= -0.403 V E° (HgS/Hg)= ? Seleccione una: a. 0.400 V b. 0.086 V O c. 0.720 V d. -.086 V e. -0.720 V||||OH 1.pTs-Cl 2. KCN/DM50 1 1. SOCl₂, pyridine 2. KOH/acetone 1. HCI 2. (CH3)3COK acetone K J
- - 144 / Natural Sciences / Chemistry And Polymer Science / Chemie zzes / Oplossingsewewig | Solubility Equilibria A solution contains 0.002 M Ag* and 1.6 x 105 M Zn2*, and the ions need to be separated. For this purpose co- is added to the solution so that both Ag,CO3 (Ksp = 8.1 x 10-12) and ZnCO3 (Ksp = 1.0 x 10-10) can precipitate from the solution. What will the concentration of co; be just before the first salt starts to precipitate. (Please give your answer with 2 significant figures.) Answer CheckAktiv Chemistry ← → C shift tab STARTING AMOUNT caps lock + esc control https://app.101edu.co ! Q X A T option Aktiv Chemistry N 2 W S #3 X 20 F3 H command 1.01 E Consider the Haber-Bosch process for the synthesis of ammonia from its elements. Calculate the theoretical yield in moles NH, from the complete reaction of 59.8 grams N₂ in the presence of excess H₂ gas according to the following balanced chemical equation: D ADD FACTOR + x( ) 2 $ 4 17.04 C g/mol N₂ POD F4 28.02 R F do 5 % -> N₂(g) + 3 H₂(g) →→→ 2NH₂(g) 2.13 g N₂ F5 V 7.04 Question 9 of 17 T G 59.8 g/mol NH, 14.01k₁ Ex. 7. A measurement of the proportion of HI decomposed in the reaction 2HI H₂ + 1₂ at k_₁ different moment of heating give the following results: Time/min ані.102 20 10 4.50 9.06 30 40 50 13.03 15.68 17.30 ∞ 21.43 Initial concentration of HI equals to 0.0446 mol dm³. Calculate the equilibrium constant of the reaction and the rate constant of the forward and the reverse reactionsThe reaction of ethanol with ethanoic acid produces ethyl ethanoate and water. CH;OH() + CH,COOH() - CH,COOC,H,(1) + H,0(1) A student suggested that the yield of ethyl ethanoate, CH,COOC,H,, could be increased by removing the water as it was formed. Explain, using the idea of K, why this suggestion is sensible.Calculate Trial I, Trial II, Trial III Vol.Ag(NO3)Added.SEE MORE QUESTIONSRecommended textbooks for youPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage LearningPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning