Mass of Beaker A + NiCl2*6H2O= 31.361g] [Volume of aqeuous en solution = 8.08 mL] [Mass if Beaker + filter paper + [Ni(en)3] Cl2 = 102.206g] [Mass of empty 50mL beaker = 28.821] [Mass of filter paper=1.056g] [Mass of empty 250mL beaker=98.663g] [Mass of NiCl2*6H2O=2.54] [Molar mass of NiCl2*6H2O=237.7] [Moles of NiCl2*6H2O=0.0107] Calculate the Percent Yield of [Ni(en)3] Cl2.

Mass of Beaker A + NiCl26H2O= 31.361g] [Volume of aqeuous en solution = 8.08 mL] [Mass if Beaker + filter paper + [Ni(en)3] Cl2 = 102.206g] [Mass of empty 50mL beaker = 28.821] [Mass of filter paper=1.056g] [Mass of empty 250mL beaker=98.663g] [Mass of NiCl26H2O=2.54] [Molar mass of NiCl26H2O=237.7] [Moles of NiCl26H2O=0.0107] Calculate the Percent Yield of [Ni(en)3] Cl2.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter1: Basic Concepts Of Chemistry

Section: Chapter Questions

Problem 43GQ: Hexane (C6H14, density = 0.766 g/cm3), perfluoro-hexane (C6F14, density = 1.669 g/cm3), and water...

See similar textbooks

Similar questions

I am trying to ascertain the density of 0.9-M HCl. The book provides a density of 1.0-M HCl as 1.016g/mL. I know the Molecular Weight aka Molar Mass is 36.46g/mol I also know that the equation to calculate the density in this instand is: Density=(Molarity x Molecular Weight)/WeightI have found examples online, and one answer provided here that shows the Density of 0.9-M HCl is 0.9115g/mL. That answer was arrived at as follows:Density = (0.9M x 36.46g/mol)/36 = 32.814/36 = 0.9115g/mL My problem is that I don't understand where the 36 came from for "weight", and I need to be able to show all unit measurements for each step. So my issue has 2 parts: 1) How was the Weight value determined to be 36 (I need to see the formula)2) Where in the step-by-step process is mL in there so that after all cancellations/conversions are completed, the only remaining units are g/mL to show how 0.9115g/mL was arrived at.
A 100 mg vitamin C tablet weighed 1.681 g. A student crushed the tablet and transferred 0.150 g of the crushed powder into a 100 mL volumetric flask, dissolved the powder in ~30 mL DI water, then filled the flask to the calibration line with DI water and mixed well to create Solution 1. The student then transferred 19.82 mL of Solution 1 into a 100 mL volumetric flask and diluted to the calibration line with DI water to create Solution 2. Calculate the expected concentration (in mM) of ascorbic acid in Solution 2. Hint: Remember that you are starting with a 100 mg vitamin C tablet.
How many grams of Mn3O4 can be obtained from 1.00 g MnO2? how many ounces of Mn3O4 can be obtained from1.00 lb MnO2? Whatwt of Mn ore should be taken so that the percentage of MnO2 in the ore can be found by multiplying by 5 to the number of centigrams og Mn3O4
A) An aqueous solution of ethyl alcohol is made by transfering 4.72 mL of liquid ethyl alcohol to a 200 . mL volumetric flask, and then adding enough water to fill the flask to the mark. What is the volume/volume percentage of ethyl alcohol in the solution? Volume/volume percentage = ________% B) An aqueous solution of acetic acid is made by transfering 17.5 mL of liquid acetic acid to a 200 . mL volumetric flask, and then adding enough water to fill the flask to the mark. What is the volume/volume percentage of acetic acid in the solution? Volume/volume percentage = ________%
A liniment contains 15 % (v/v) of methyl salicylate. How many mL of the liniment can be made from 1 pint of methyl salicylate? Volume(ml) x %(expressed in decimal)= mL of active ingredients
a sample of unknown mixture has a total mass of 134g, a total volume of 113 cm3, and consists only of an unknown A (density=1.4 g/cm3) and B (density=1.122g/cm3). what is the volume of component B in this mixture? Assume that the volumes are additive.
A cylindrical bar was found at the bottom of a storage tank of unknown composition. The material had a diameter of 8 mm, a length of 62 cm and a mass of 0.018 kg. What is the density of this material in g/mL? The volume of a cylinder is given by V = πr^2h.
Sucrose solution for experiment 1: (Question a-c)Prepare a solution of sucrose by accurately weighing 9.0 – 9.25 g of sucrose into a 100mLbeaker / conical flask. Record the mass of the sample. Add 25 mL distilled water. Mix until allcrystals dissolve.NaCl solution for experiment 2: (Question d-f)Prepare a solution of NaCl by accurately weighing approximately 1.5 g of NaCl into a 100 mLbeaker / conical flask. Record the mass of the sample. Add 25 mL distilled water. Mix until allcrystals dissolve.MgCl2٠6H2O solution for experiment 2: (Question d-f)Prepare a solution of magnesium chloride by accurately weighing approximately 3.6 g ofMgCl2٠6H20 into a 100 mL beaker / conical flask. Record the mass of the sample. Add 25 mLdistilled water. Mix until all the crystals dissolve
What volume of iron (7.87 g/cm3) would be required to balance a 1.25 cm3 sample of lead (density 11.4 g/cm3) on a two-pan laboratory balance?
The average micro-nano plastic concentration in bottled water was about 2.4×10^5 particles per liter of bottled water, about 90% of which were nano-sized particles. Assuming that each nanoparticle can be approximated as a sphere with a diameter of 100 nm and that the average density of nanoparticles is 1.2 g/cm^3, estimate the mass of nanoparticles ingested if someone drinks all of their recommended 64 fluid ounces of water per day via bottled water every day for a year. Provide your answer is units of nanograms (ng).
two strips of metal each weighing 100g are placed into a cylinder containing water. The volume of water displaced is 8.8 ml in one case and 37.0ml in the other case. identify the two metal strips. AU Fe Al Pb Ag 19.3 7.9 2.7 11.3 10.5 * For this question do i have to do any calculations? Or just state that Fe is Iron, Ag is silver etc.? Which weighs the most, 10cm3 of iron or 5.0cm3 of silver?
Given the following data for Mass of test tube and stearic acid = 14.17 gMass of test tube = 11.40 gFreezing point of strearic acid = 69.59o CMass of weighing paper + naphthalene =1.230 gMass of weighing paper = 0.920 gFreezing point solution = 64.00o CKf = 4.5o C/m Determine the following1. mass of stearic acid in g (2 decimal places); 2.77g2. mass of naphthalene in g (2 decimal places); 0.31g3. freezing point depression (2 decimal places); 3.93oC4. molality of solution (3 significant figures); _____5. moles of naphthalene (3 significant figures); _____6. molar mass of naphthalene, experimentally (3 significant figures); _____7. % error if theoretical molar mass of naphthalene is 128.17 g/ mole, USE ABSOLUTE VALUE (3 significant figure); _____