7.CaCO3 CaO + CO2 8.P4 + 3 02 →2 P203 9. 2 RBNO3 + BeF2 Be(NO3)2 + 2 RbF 10.C3H60 + 4 02 3 CO2 + 3 H20 11.2 AgNO3 + Cu 12. SeC16 + 02 Cu(NO3)2 + 2 Ag SeO2 + 3C121
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- Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 10. What is the ∆S⁰ in the combustion of hydrogen in the presence of excess oxygen yields water: 2H2(g) + O2(g) → 2H2O(l) in J/K?Sample: Commercial bleach Technical specifications:- Composition: sodium hypochlorite (NaClO) and demineralized water;- Active chlorine content: 2.00 to 2.50% (m/m);- Active ingredient: sodium hypochlorite (NaClO).- Approximate density: 1.08 g/ml;- Physical Aspect: Liquid;- Color: Colorless. Note: the active chlorine content refers to the chlorine gas produced from the following reaction:ClO¯ + Cl¯ + 2H+ ⇋ Cl₂(g) + H₂OData:M.A.: H = 1.0079 g/mol; Na = 22.989769 g/mol; S = 32.065 g/mol; I = 126.90447 g/mol; O = 15.9994 g/mol; Cl = 35.453 g/mol. Material available in the laboratory's warehouse: Reagents:Distilled water; standardized solution of sodium thiosulfate (Na₂S₂O₃), at a concentration of 0.0500 mols/L; 20% KI solution; glacial acetic acid and; starch gum (indicator). Glassware:Bechers of all sizes available on the market; 50, 100, 150, 200 and 250 ml Erlenmeyer flasks; 10.00 and 25.00 mL volumetric pipettes; 25.00 mL burette; 25.00, 50.00 and 100.0 mL volumetric flasks. Calculate…A scientist was tasked to extract Fe from an aqueous suspension that contains 106 g of Fe2O3. The following steps detail the transformation of Fe2O3 (aq) to elemental iron: I. Enough sulfur trioxide gas was bubbled to Fe2O3 aqueous suspension to completely yield ferric sulfate. II. Then, 5.00 M nitric acid was added to ferric sulfate yielding an aqueous solution of ferric nitrate. III. Excess magnesium powder was added to the aqueous solution of ferric nitrate precipitating the solid iron ----- a. Write the balanced chemical reaction and the type of chemical reaction for [I], [II], [III]. Do not forget to indicate the states of the reactants and products (s, l, g).(CHOICES: COMBINATION, SINGLE DISPLACEMENT, DOUBLE DISPLACEMENT) b. What is the final mass of iron? Express final answers in 3 significant figures. c. High-concentration HCl is supposed to be added at the last part of the procedure. Briefly state its purpose.
- 13.Using the thermodynamic values provided in Appendix G (Links to an external site.) calculate ΔG°rxn in (kJ/mole) for the following reaction. 2 CH3OH(l) + 3 O2(g) →2 CO2(g) + 4 H2O(l) Group of answer choices A, 2070 B, 1404 C, -2070 D, 465 E, -1404Calculate ΔG. For the following process at 25°C: BaF2 (s) = Ba2 + (aq) + 2F - (aq) The Ksp of BaF2 is 1.7 x 10^-6 ΔG° = _____ kJ/mol1) Gibbs free energy of the formation of one mole of pure TiO2 (s) from pure Ti (s) and pure oxygen gas is given as: Ti (s) + O2 (g) = TiO2 (s) ΔG°TiO2 = - 446230 + 88.9 T J/mole Discuss, based on calculations, whether Ti can be oxidized inside a heat-treatment furnace, which works at 1024 °C and 1 atm air (oxygen and nitrogen mixture) pressure.
- The chief chemist of the Brite-Metal Electroplating Co. isrequired to certify that the rinse solutions that are discharged from the company’s tin-plating process into the municipal sewer system contain no more than 10 ppm (parts per million) by mass of Sn2+. The chemist devises the following analytical procedure to determine the concentration. At regular intervals, a 100-mL (100-g) sample is withdrawn from the waste stream and acidified to pH = 1.0. A starch solution and 10 mL of 0.10 M potassium iodide are added, and a 25.0-mA current is passed through the solution between platinum electrodes. Iodine appears as a product of electrolysis at the anode when the oxidation of Sn2+ to Sn4+ is practically complete and signals its presence with the deep blue color of a complex formed with starch. What is the maximum duration of electrolysis to the appearance of the blue color that ensures that the concentration of Sn2+does not exceed 10 ppm?The free energy of the combustion of oxalic acid HC2H3O2 at 25.0 ºC is -246.05 KJ/mol. What is the equlibrium constant Ka at 25ºC?1. What is the standard free energy change for the reaction below? Is the reaction expected to bespontaneous under standard conditions?FeS(s) + O2(g) → Fe(s) + SO2(g) 2. Use the thermodynamic data provided value from the Table: to calculate the equilibriumconstant for the dissociation of dinitrogen tetroxide at 25 °C.2NO2(g) ⇌ N2O4(g)
- Calculate Kat 298 K for each reaction:(a) MgCO₃⇌Mg²⁺(aq)+ CO₃²⁻(aq)(b) 2HCl(g) +Br₂(l) ⇌ 2HBr(g) +Cl₂(g)(c) H₂(g) +O₂(g) ⇌ H₂O₂(l)Pyrite (FeS2) is often roasted to obtain sulfur dioxide for making sulfuric acid. Consider the roasting reactionFeS2 + O2 = Fe2O3 + SO2Stoichiometric exercises:a) Formulate the correct stoichiometric roasting reaction Calculate, in respect to 1 t of pyrite, the stoichiometric amounts ofb) Oxygen required for roasting (in m3) c) Obtained hematite by-product (in t) d) Sulfur dioxide produced (in m3) Thermodynamic considerations:e) Calculate the reaction enthalpy ∆Ho298 for the above roasting reaction (in MJ/t of pyrite) Mind you: Requested is the reaction enthalpy per 1 t of pyrite! f) State whether the reaction is exo- or endothermic and say why. g) Calculate the actual change of entropy ∆So298 in J/(mol K) and explain why it is positive or negativeUse data from CRC_Std_Thermodyn_Substances and CRC_Std_Thermodyn_Aqueous-Ions to calculate ΔrH∘ΔrH∘ (in kj/mol) for the following at 25 ∘∘C. 2CaC2O4(s)⟶4CO(g)+O2(g)+2CaO(s)