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Insert correct coefficients to balance.
a.) S + 6HNO3 ------> H2SO4 + NO2 + H2O
b.) 3Cu + 8HNO3 ------> Cu(NO3)2 + NO + H2O
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- i have hard time geting it stright even after I do the experiment can u help me with the one pls Material ChemicalsSealed NO2 tubes, KSCN solution (0.002 M), acidified Fe(NO3)3 solution (0.2 M), KSCN crystals, Fe(NO3)3 crystals, KOH (concentrated (8 M)), distilled waterApparatus:Bunsen burner, ring stand, wire gauze, matches, thermometer, dropper, test tubes, glass stirring rod, beaker tongs Procedure Part A: Fill a 600 mL beaker to the 3/4 mark with water. Bring to a boil using a Bunsen burner. In another 600 mL beaker, fill to the 1/2 mark with water; add ice in order to lower the temperature to about 0°C. Note the room temperature. Observe the NO2 thoroughly at room temperature. Place the sealed NO2 tube in the cold bath. Note your observations. Remove the test tube from the cold bath. Let the test tube stand until it reaches room temperature. Note your observations. Place the test tube in the hot bath. Note your observations. Remove the test tube from the hot bath. Let the test…An impure sample of 0.1002 g benzoic acid underwent purification by recrystallization. A mass of 0.0542 g of white solid benzoic acid was obtained. Calculate the % purity of the initial sample. Show calculations and report the result with correct number of significant figures. Hi there please answer all parts clearly and concisely with legible hand writting, thank you!Molarity: 0.148 M Na2S2O3 Data for Unknown Sample Trial 1 Trial 2 Mass of Sample 0.081 g 0.083 g Volume of Na2S2O3 ----------------- ------------------- Final Buret Reading 0.78 mL 0.84 mL Initial Buret Reading 0.07 mL 0.10 mL Net Volume of Na2S2O3 _____mL ______mL Calculation of Percentage NaOCl -------------- ------------- Moles of Na2S2O3 used _______mol _______mol Moles of NaOCl reacted _______mol _______mol Mass of NaOCl in sample _______g _______g Percentage by weight NaOCl (g NaOCl/g sample) X 100% _______% _______%
- Given the following data, what is the molarity? Include the relative error Error is 1.0 mg or 1.0e-4using exactly 5.00 mL of 0.0400 M stock CuSO4 solution. Add 100 mL of water. Data for Part IMass of empty dish: 32.470 g empty dishVolume of 0.0400 M solution: 5.00 mL CuSO4 solution.Mass of dish and 0.0400 M solution: 37.497 g dish and solutionMass of dish and CuSO4 solid: 32.503 g dish and CuSO4 solidCalculations for Part I1. Calculate the mass of solution2. Calculate the mass of solid CuSO4 dissolved in the solution.3. Calculate the number of moles of solid CuSO4 dissolved in the solution.4. Calculate the mass of water evaporated from the solution.5. Calculate the density of solution, (g solution/mL solution).6. Calculate the % by mass, CuSO4 in solution (100 x g CuSO4/g solution).7. Calculate the molality of solution (moles CuSO4/kg solvent).8. Calculate the molarity of solution (moles CuSO4/L solution).9. Given that the true molarity is 0.0400 M, calculate the percent error of your result.I got a task in analytical chemistry to calibrate, standardize, verify and validate an analytical balances, can you help me?
- mass of dish 1631.5 g mass of dish and mix 1822 g mass of dish and agg. after extraction 1791g mass of clean filter 25 g mass of filter after extraction 30 g mass of agg. in 150 ml solvent 1.2g if Ac% 5% find the volume of the solventUsing a 25mL pipette, you prepare a standard solution by pipetting 25.00mL of the standard iron solution[0.25g/L] into a 500mL volumetric flask. Then, using a 10mL pipette you transfer a 4mL aliquot of this solution into a 50mL volumetric flask and dilute up to the mark. Calculate the % uncertainty.9. The method described in Problem 5-8 is to be used for the analysis of ores that assay about 1.2% gold. What minimum sample mass should be taken if the relative error resulting from a 0.4-mg loss is not to exceed(a) -0.1%? (b) -0.4%? (c) -0.8%? (d) -1.1%? Here is the number 5-8 5. Describe at least three ways in which a systematic error might occur while using a pipet to transfer a known volume of liquid.6. How are systematic method errors detected?7. What kind of systematic errors are detected by varying the sample size?8. A method of analysis yields masses of gold that are low by 0.4 mg. Calculate the percent relative error caused by this result if the mass of gold in the sample isa. 500 mg. b. 50 mg. c. 150 mg.d. 70 mg.
- using exactly 5.00 mL of 0.0400 M stock CuSO4 solution. Add 100 mL of water. Data for Part IMass of empty dish: 32.470 g empty dishVolume of 0.0400 M solution: 5.00 mL CuSO4 solution.Mass of dish and 0.0400 M solution: 37.497 g dish and solutionMass of dish and CuSO4 solid: 32.503 g dish and CuSO4 solidCalculations for Part I1. Calculate the mass of solution? 5.027 g 2. Calculate the mass of solid CuSO4 dissolved in the solution? 0.033 g 3. Calculate the number of moles of solid CuSO4 dissolved in the solution? 2.07 x 10-4 mol4. Calculate the mass of water evaporated from the solution? 0.0414 M5. Calculate the density of solution, (g solution/mL solution)?6. Calculate the % by mass, CuSO4 in solution (100 x g CuSO4/g solution)?7. Calculate the molality of solution (moles CuSO4/kg solvent)?8. Calculate the molarity of solution (moles CuSO4/L solution)?9. Given that the true molarity is 0.0400 M, calculate the percent error…Show your work: Balance the following chemical equation: C7H16 + O2 ---> CO2 + H2OWhat is an analytical balance?