The reaction of chlorine dioxide with basic water is 2C1O2(aq) + 2OH-(aq) → CIO2-(aq) + CIO3-(aq) + H2O(1) [ClO₂] [OH-¹] -A[CLO2]/At (M/s) 1 2 3 1. Exp't (M) (M) (M s¹) 0.0500 0.100 5.75x10^-2 0.100 0.100 2.30x10^-1 0.100 0.0500 1.15x10^-1 2. 1.Determine the order of reaction with respect to reactant CIO2 Determine the order of reaction with respect to reactant OH 3. Determine the rate constant 4. The rate of the reaction when [CIO2] = 0.12 M and [OH-] = 0.05 M
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- 1) Commercial fuming Sulphuric acid (Oleum-H2S2O6) is 99.9% solution. Please convert it into molarity.2) Find out the Volume (dm3) of product (gas) at RTP when 0.58 M, 150 mL NaOH (aq.) reacts with 350 mL, 0.25 NH4Cl.The volume of HCI is 100 mL , mass of solid added is 1.008g, moles of solid 0.0276 Mol, mass of HCI is 100g, initial temperature is 21.8 degrees Celsius, Final temperature is 30.7 degrees Celsius, Calculate q rxn(= -mc Delta T of HCI),1) Mass of flask, aluminum foil, and rubber band 68.45g 2) Temp. Of boiling, water 98.20 0C 3) Barometric pressure 755 mmHg 4) Volume of flask (volume of vapor occupies flask) 152 ml 5) Mass of flask, aluminum foil, rubber band, and condensed vapor 68.60g 6) Mass of condensed vapor is (5)-(1) Find Molecular weight of unknown ______ g / mol Calculation PV = (m/M)RT) è M = (mRT) / PV = ? Unknown liquid- Based on Molecular weight determine which unknown below has this molecular weight: Methanol, Ethanol, Isopropanol, Propanol. UNKNOW IS : __________________________
- An important process for the production of acrylonitrile (C3H3N) (U.S.production is greater than 109 lb) is given by the following reaction: 2C!H"(?) + 2NH!(?) + 3O#(?) H⎯⎯⎯J 2C!H!N(?) + 6H#O(?)A 150.-L reactor is charged to the following partial pressures at 25°C: ? = 0.500 MPa? = 0.800 MPa ? = 1.500 MPa What mass of acrylonitrile can be produced from this mixture (MPa = 106 Pa)?An aqueous waste stream that has a maximum concentrationof 0.50 M H₂SO₄ (d=1.030 g/mL at 25C) will be neutralized by controlled addition of 40% caustic soda (NaOH; d=1.430 g/L) before it goes to the process sewer and then to the chemical plant waste treatment facility. However, a safety re-view finds that the waste stream could meet a small stream of animmiscible organic compound, which could form a flammable vapor in air at 40.°C. The maximum temperature of the causticsoda and the waste stream is 31°C. Could the temperature in-crease due to the heat of neutralization cause the vapor to ex-plode? Assume the specific heat capacity of each solution is 4.184 J/gK.Use only the first decimal points (X.X) for atomic masses. R = 8.314 L*kPa/mole*K. In a reactor at 350.0 kPA and 95 °C, HCl adds to acetylene by the following reaction:2HCl(g) + C2H2(g) --> C2Cl2H4(g)39.1 g of HCl and 39.1 g of acetylene are placed into the reactor. What is the limiting reagent? What is the final volume of the system?
- (a) A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas City (MCI) to Baltimore (BWI) burned 11,800 lb (about 1700 gallons) of Jet A fuel en route. Jet A fuel is kerosine based, consisting primarily of CnH2n+2 hydrocarbons, with n =6 to 16, so the carbon:hydrogen ratio is close to 1:2. During this flight, how much CO2 was released into the atmosphere? Assume the combustion of the fuel was complete, so all the fuel was burned to form CO2 and H2O. Give both the mass of CO2 produced (in kg and in lbs) and the volume it would occupy at 298 K, 1 atm.(b) How much CO2 would be released into the atmosphere if those passengers and crew made the trip instead, in pairs, in hybrid cars at 40 miles per gallon. Assume the density of the gasoline is 0.75 kg L-1 and that carbon and hydrogen dominate the composition in a ratio of 1:2. The road trip is 1082 miles.One way to determine the hardness of a water sample is to precipitate the calcium out of solution as a carbonate. The net ionic reaction for this precipitation is: Ca2+(aq) + CO32-(aq) → CaCO3 (s) A 1.00 L sample of water is drawn from a Phoenix, AZ well and 0.534 g of calcium carbonate is recovered using the above reaction. What was the Ca2+ concentration of the original water sample in ppm? Show your work and include units. Hint: ppm stands for parts per million, and in the case of an aqueous solution, this is equivalent to mg/L.Use only the first decimal points (X.X) for atomic masses. R = 8.314 L*kPa/mole*K . In a 2.50 L reactor at 27 *C, sodium oxide captures CO2 from the gas phase by the following reaction:Na2O(s) + CO2(g) --> Na2CO3(s)36.2 g of Na2O(s) and 26.1 g of CO2(g) are placed into the reactor. What is the limiting reagent? Na2O(s) CO2(g) What is the final pressure of the system? kPa
- In an experiment, sulfuric acid reacted with different volumes of sodium thiosulfate in water. A yellow precipitate was formed during the reaction. A cross drawn at the base of each flask became gradually invisible due the formation of this yellow precipitate. The time taken for the cross to become invisible was recorded. A partial record of the experiment is shown. Experimental Record Flask Volume ofH2SO4 Volume ofSodium Thiosulfate Volume ofWater Time 1 5 mL 50 mL 0 mL 19 seconds 2 5 mL 40 mL 10 mL 3 5 mL 30 mL 20 mL 4 5 mL 20 mL 30 mL Based on your knowledge of factors that affect the rates of chemical reactions, predict the trend in the last column of the experimental record. Use complete sentences to explain the trend you predicted. You do not have to determine exact values for time; just describe the trend you would expect (increase or decrease) and why it occurs.Combustible vapor-air mixtures are flammable over a limitedrange of concentrations. The minimum volume % of vapor thatgives a combustible mixture is called the lower flammable limit(LFL). Generally, the LFL is about half the stoichiometric mix-ture, the concentration required for complete combustion of thevapor in air. (a) If oxygen is 20.9 vol % of air, estimate the LFL forn-hexane, C₆H₁₄. (b) What volume (in mL) of n-hexane (d=0.660 g/cm³) is required to produce a flammable mixture of hexane in 1.000 m³of air at STP?Butane (C4H10)(C4H10) and dry air are fed to a combustion reactor at a steady rate of 45.9 mol/s45.9 mol/s butane and 2500.0 mol/s2500.0 mol/s dry air. Assume the butane reacts completely to produce CO2CO2 and H2O.H2O. The reactants enter the reactor at 25 ∘C25 ∘C and the products leave the reactor at 1110.4 ∘C.1110.4 ∘C. Calculate the percent excess air. Using the information below, find the heat interaction. Species ΔHf at 298 K(kJ/mol) CP (kJ/kmol·K) O2 0 3.5R N2 0 3.5R C4H10 -125.5 12R CO2 -393.5 3.5R H2O -241.8 3.5R