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- Calcium Chloride Ammonium Chloride Trial 1 Trial 2 Trial 3 Trial 1 Trial 2 Trial 3 Mass of water 100g 100g 100g 100g 100g 100g Mass of salt 5.36g 10.28g 15.10g 5.29 10.43 15.31 Moles of salt Initial T 21.0 21.0 21.0 20.0 20.0 20.0 Final T 29.6 36.2 43.5 17.1 13.2 10.1 ΔT 8.6 15.2 22.5 -2.9 -6.8 -9.9 ΔH(Joules) ΔH(kj/mol)Calculate the density in molecules/cm3 for a gas at 10 torr and at 1 x 10-7 torr. 10-7 torr is the typical pressure in a mass spectrometer. show work please :)A. B. and C. already solved (https://www.bartleby.com/questions-and-answers/chemistry-question/a89691d6-2162-4677-b0cc-dc84fcceda08). Please answer E, F and GCircle in pencil in the image on th eirght cide of the diagram is a "2"( Pb(NO3)2 ).
- To determine the mass of Fe2O3 from the given mass of K3Fe(CN)6, the gravimetric factor to be used is a. Fe2O3 / K3Fe(CN)6 b. Fe2O3 / 2K3Fe(CN)6 c. 2Fe2O3 / K3Fe(CN)6 d. 3Fe2O3 / 2K3Fe(CN)6Aleks data for AgBrO3 is 5.38 x 10^-5Produce Water mass “X” is known to be a mixture of water masses “1”, “2”, and “3”. Using the data plotted below, calculate the composition of “X” (i.e. determine the fraction from each of the 3 water masses that makes up water mass X). Watermass#1– SF6 =25 S=33.5 Watermass#2– SF6 =75 S=32 Watermass#3– SF6 =50 S=36.5 Water mass X – SF6 =60 S= 34
- How to manipulate formula mgh=1/2mv2 to find velocity and massBeaker 0.00200 M Fe(NO3)3, mL 0.00200 M NaSCN, mL total volume, mL 1 3.000 2.000 10.00 2 3.000 3.000 10.00 3 3.000 4.000 10.00 4 3.000 5.000 10.00 5 (blank) 3.000 0.000 10.00 In Solutions 1-4 you are adding successively larger volumes of 0.00200M SCN- to the Fe3+ solution and diluting to 10.00 ml. Calculate the final diluted molarity of SCN- in solution #1 Your answer should have 3 sig figs =1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)pls compelete the 2nd table given the data
- pls complete the 2nd table given the data1. 500.0 mL 0.2 M KI2. 500.0 mL 0.2 M KCl3. 500.0 mL 0.1 M K2S2O84. 500.0 mL 0.1 M K2SO45. 500.0 mL 4.0 mM Na2S2O3 (from Na2S2O3∙5H2O)"Nitric acid reacts with S to give H2SO4 and nitrogen monoxide. 30 ml of acid at 25% by mass and a density of 1.08 g/ml with 5 g of S. a) Adjust the reaction. b) Calculate limiting reactant and its excess. c) Calculate mass of unreacted reactant. d) Determine volume of NO at 600 mm Hg and 20°C. 20% yield"THE EQUATION THEY PROVIDE IS:2HNO3 + S → H2SO4 +2NOYOU DONT NEED TO ADD H20 IN THE EQUATIONStock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.