15- The reaction given below is not balanced. If 12 moles of nitrogen were produced in a reaction, how many moles of copper would be produced simultaneously ? NH3 + Cuo ------> Cu + N2 + H2O a) Cannot be calculated without knowing the amount of reactants. 12 mol 36 mol 6 mol Boş bırak
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- 7. Consider a1Msolution ofNa3AsO4. Write the charge and mass balance equations for this system. (please type answer not write by hend)A 100 ml sample of pond water was analyzed using Winkler method to determine its oxygen demand. It took 32.4 ml of 0.0100 M Na2S2O3 to react with Iodine. Calculate the oxygen for this pond water.Please answer all parts! Background: 1. The rate of the reaction A + 3B → C + 2D was reported as 2.7 M/sec. Calculate the rates of formation and consumption of each of the reactants and products. (include negative signs where appropriate). 2. The rate of the following disproportionation redox reaction was studied by monitoring the rate of formation of MnO4- 3 MnO42- (aq) + H+(aq) --> 2 MnO4-(aq) + MnO2(s) At the 5.30 minute mark of the reaction the concentration of MnO4- was found to be 0.52 M. At the 6.25 minute mark of the reaction the concentration of MnO4- was found to be 1.75 M. a. What is the rate of appearance of MnO4-?b. What is the rate of disappearance of MnO42-?c. the rate of formation of MnO2 is how many times the rate of formation of MnO4-?d. What is the value of the rate of reaction?
- Toluene, C7H8 , is burned with 30% excess air. A bad burner causes 15% of the carbon to form soot (pure C) deposited on the walls of the furnace. What is the Orsat analysis of the gases leaving the furnaceThe mercury in a 0.8142-g sample was precipitated with an excess of paraperiodic acid, H5IO6: 5 Hg 2+ + 2 H5IO6 ---> Hg5(IO6)2 (s) + 10 H + The precipitate (MW = 1448.8 g/mol) was filtered, washed free of precipitating agent, dried, and weighed, and 0.4114 g was recovered. Calculate the a) % Hg (200.6 g/mol) b) % Hg2Cl2 (472.1 g/mol)Which of the following are equivalent to 2,500 ppm Cu2+? (There may be more than one answer) MW: Cu (63.55) a) 2.5 ppb Cu2+ b) 2,500,000 ppb Cu c) 2.5 ppt Cu2+ d) 39.34 mM e) 0.03934 M f) 0.07868 N (in precipitation reaction) g) 0.07868 N (in redox into Cu+)
- Assuming an efficiency of 32.70%,32.70%, calculate the actual yield of magnesium nitrate formed from 145.4 g145.4 g of magnesium and excess copper(II) nitrate. Mg+Cu(NO3)2⟶Mg(NO3)2+CuWhen a sample of the aqueous layer with a volume of 12.25 mL is collected, it requires 18.87 mL of a titrant solution of S2O32- with a concentration of 0.01617 M to reach the endpoint. The reaction has a 2:1 mole ratio of thiosulfate to all reducible iodine species. Calculate the concentration of total reducible iodine (in mol/L) in the aqueous layer. Include only the numerical answer (no units).Calculate the time, in minutes, needed to plate 17.697 g of metal M at 43 Amps. The molar mass of metal M is 57.915 g/mol. M6+ + 6 e– → M Recall that, C = A*s, and Faraday’s constant, F, is 96,485 C/mole of electrons.
- Please Help!! Part A: Electrochemical Cell Mass Data for Electochemical Cell Copper Zinc Initial mass of strip (g) 2.421 2.436 Final mass of strip (g) 2.602 2.250 Measured Ecell (V)= 1.02 Part B: Electroplating Mass Data for Electoplating Mass (g) Initial 0.930 After first plating 1.083 After second plating 1.238 After third plating 1.377 Part A: Electrochemical Cell Table view List view Mass Calculations for Electochemical Cell Copper Zinc Initial mass of strip (g) 2.421 2.436 Final mass of strip (g) 2.602 2.250 Mass gained(+) or lost(−) (g) 0.18 -0.19 what is Computed Ecell (V)? what is Computed ΔG (kJ/mol)? Mass Calculations for Electroplating (fill in chart) First Second Third Final mass of paper clip (g) 1.083 1.238 1.377 Initial mass of paper clip (g) 0.930 1.083 1.238…Part A: Electrochemical Cell Mass Data for Electochemical Cell Copper Zinc Initial mass of strip (g) 2.709 3.111 Final mass of strip (g) 2.097 2.909 Mass gained or lost (g) 0.198 -0.201 Measured Ecell (V)= 1.19 Part B: Electroplating Mass Data for Electoplating (measurements taken every 5 min) Mass (g) Mass Gained Initial 0.948 0 After first plating 1.094 0.146 After second plating 1.244 0.296 After third plating 1.402 0.454 a) Using the amount of zinc lost in part A, how much copper should have theoretically been gained? b) What is ther average weight of copper gained per minute in part B of this expirement? c) What is the present by mass of copper on the paper clip at the end of this expirement? How many minutes would it take the paper clip to be 50% copper?HURRY ASAP I WILL RATE NO NEED FOR EXPLANATION WHICH OPTIN Which oxidizing agent do you use to apply the following conversions? HOCH2CH2CH2CH2CH2OH --- HO2CCH2CH2CH2CO2H KМn04, 0H-,ısı РСС/СН2Сl2 H2, Pt NaBH4 LiAlH4