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I cant figure out which is the last part of the problem, solving for Δ? ( Determine the entropy change when 8.50 mol HBr(l)8.50 mol HBr(l) freezes at atmospheric pressure)
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- 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 negative1) 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.Silver chromate (Ag2CrO4) is a red solid that dissolves in water to the extent of 0.029 g L-1 at 25°C. Estimate its Ksp and compare your estimate with the value in Table 16.2.
- Using the thermodynamic data provided below, calculate Ksp for ZnS(s) at 25°. ΔH°f (kJ/mol) S° (J/K·mol) Zn2+(aq) –152.4 –106.5 S2–(aq) 41.8 22 ZnS (s) –203 57.7Calculate the E0 for the reaction between S2- and Fe3+ that yields SO42- and Fe2+. Standard Gibbs Free energies as follows... S2- …….85.9 Fe3+……-8.56 Fe2+……-82.88 So42-……-744.0 This was all the information I was given. Thank you for helping me understand!1. Why do we compute for TFM in soaps. How does one calculate for TFM? 2. Describe the difference between a laundry soap and a toilet soap? What are the basic ingredients of laundry soap and toilet soap.
- why does enrgy have to be supplied to a chemical in order to break the IMFs between the molecules in that chemical?A sample of feldspar weighing 1.500g is decomposed, and eventually there is obtained a mixture of KCl and NaCl weighing 0.1801 g. These chlorides are dissolved in H2O, a 50-mL pipetful of 0.08333 N AGNO3 is added, and the precipitate is filtered off. The filtrate requires 16.47 mL of 0.1000N KCNS, with ferric alum as indicator. Calculate the percentage of K2O in the silicate.Given below (c): Standard gibb's free energies (∆Gf0 kJ mol-1 ): UO2 = -962.7 UO22+ = -953.5 U4+ = -579.1 Fe2+ = -78.9 Fe(OH)3 ferrihydrite = -692.07 Mn2+ = -288.1 MnO2 pyrolusite = -465.1 HS- = 12.1 H+ = 0 H2O = -237.1 S0 = 0 Given: U(VI) as uraninite; UO2 (where Mn2+ = reductant; MnO2 pyrolusite = product): ∆ Gr0 = -21.3 KJ/mol E0 (emf) = 0.110 V n = 2 F = 96.42 QUESTION: Calculate Eh equation below to calculate at different pH: – Eh = E0 + (RT/nF) * lnK For U(VI) as uraninite; UO2 (where HS- = reductant; S0 = product): UO22+ + Hs- ---- > UO2 + S + H+ [A] pH 3 [B] pH 7
- 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.Calculate the [Cu2+] and [IO3–] in a solution made by saturating pure water with solid Cu(IO3)2. Use your mean Ksp value above when performing the calculation. Mean Ksp=0.050From Elements of CRE by Fogler - 2016