Show the process of copper electroless plating on iron rod using EDTA stabilized copper sulphate and formaldehyde as reducing agent is a apontaneous process. (E^0 Cu/Cu^2+ = +0.216V, E^0 OH-/H2O = -1.14V %3D
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Q: Give example of sacrificial anodes and noble coating, define the two and give practical application
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Q: The standard electrode potential for the reduction of the Cu complex of EDTA is given by CuY-2…
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Q: Show the process of copper electroless plating on iron rod using EDTA stabilized copper sulphate and…
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- Show the process of copper electroless plating on iron rod using EDTA stabilized copper sulphate and formaldehyde as reducing agent is a apontaneous process. (E^0 Cu/Cu^2+ = +0.216V, E^0 OH-/H2O = -1.14V)What are the maximum atomic and weight percentages of Cu that can be added to Au without exceeding a resistivity that is thrice that of pure gold? (Alloys are normally prepared by mixing the elements in weight. Resistivity of Au at 0°C is 20.5 nΩ m Nordheim coefficient for Cu in Au at 20°C is C = 450 nΩ m. Resistivity of Au at 20°C, using α0 = 1/242 K-1 )Resistivity measurements at 300 K show that an annealed metal single crystal has amonovacancy concentration CV = 10-9. When the same crystal is quenched from a hightemperature, the measurements indicate CV = 2x10-3. Calculate the temperature of thequench [Take Hf = 51.4 kJ/mol and R = 8.314 J/mol.K]. State any assumption involved. (5)(b) Explain why the esistivity of a metal is expected to be found more at room temperature after quenching. Hint: Use Matthiessen’s rule (find out by self-studying and cite thesource.)
- 1.065 g of stainless steel was dissolved in hydrochloric acid (chromium as Cr 3+ ) and diluted to 500.0 ml. A 50.00 ml sample was passed through a Walden reducer, where only iron is reduced (Fe3+ + e- Fe2+), and titrated with 0.01920 M KMnO4 solution, which consumed 13.72 ml. A 100.0 ml sample was passed through a Jones reducer (Cr3+ + e- Cr2+ and Fe3+ + e- Fe2+) into 50.00 ml of a 0.1000 M Fe3+ solution. The resulting solution was titrated with 0.01920 M KMnO4 solution and 36.43 ml was consumed. Calculate the Fe and Cr concentrations of the sample in weight percent.a. An iron ore has a 55% Fe2O3 with 5% moisture content. What is the Percentage of Fe2O3 in a dry basis? b. An iron ore has a 55% Fe2O3 with 5% moisture content. What is the Percentage of Iron in a dry basis?Give example of sacrificial anodes and noble coating, define the two and give practical application
- AZ91 alloy; a) What is its chemical composition? b) Which of the strength increasing methods are suitable and which are not? Explain c) Is nitration suitable as one of the surface hardening methods? Please explain9 The pyrite (iron sulfide) roasting process is carried out following the next reaction [FeS2 (s) + O2 (g)]25°C → [Fe2O3 (s) + SO2(g)] 900 °C a) Determine the enthalpy balance for the reaction as stated in the reaction shown b) Determine the enthalpy balance using air with 10% excess and preheated to 500°CIs it posible to remove 99% of 1.0 μM CuY2- impurity (by reduction to solid Cu) from a 10.0 mM CoY2- solution at pH 4.0 without reducing any cobalt? Here, Y (actually, Y4-) is EDTA and the total concentration of free EDTA is 10.0 mM. Hint: Concepts of Equilibrium of EDTA Complex Formation are involved in the solution of this problem. Standard reduction potentials to use in this problem are:CuY2- + 2e- ➙ Cu(s) + Y4- E°= -0.216 VCo2+ + 2e- ➙ Co(s) E°= -0.282 V.
- Copper is produced from chalcopyrite concentrate from a mixed type ore containing 1.2% CuFeS2 (chalcopyrite) and 6% Cu3 (CO3) 2 (OH) 2 (azurite) by sulfating roasting leaching method. 4 tons of chalcopyrite concentrate is roasted daily. If it is assumed that the amount of iron in the solution is 20% under the same conditions, how much copper is produced in 1 day?A 25.0 mL sample containing Fe3+ was treated with 10.00 mL of EDTA0.0367 mol / L to complex all the iron and leave an excess of EDTA insolution. To the excess of EDTA was added 2.47 mL of Mg2+ 0.0461 mol / Lwhich guaranteed all EDTA consumption. What was the concentration of Fe3+ in the original solution?(a) What is the percentage of MnO2 in a pyrolusite ore if a sample weighing 0.4000 g is treated with a 0.6000 g of pure H2C2O4.2H20 and dilute H2SO4 and after reduction has taken place (MnO2 + H2C2O4 + 2H+ Mn2+ + 2CO2 + 2H2O), the excess oxalic acid requires 26.26 mL of 0.1000 N KMNO4 for titration? (b) If pure As2O3 were used instead of oxalic acid, how many grams would be required in order for the other numerical data to remain the same?