SOLVE THE FOLLOWING PROBLEM AND SHOW YOUR COMPLETE AND DETAILED SOLUTIONS Calculate the number of grams of Ca3(PO4)2 and the number of grams of excess reagent and limiting reagent in each of the following: 3CaCO3 + 2H3PO4 → Ca3(PO4)2 + 3C02 + 3H₂0 a. From 3.25moles of CaCO3 and 475g of H3PO4.
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- Vanadium(V) oxide reacts with calcium according to the chemicalequation below. When 20.0 moles of V20s are mixed with 20.0moles of Ca, which is the limiting reagent in the production of V(I)?V20s (s) + 5Ca(1) -> 2V(1) + 5CaO(s) a. CaOb. Vc. No reagent is limiting.d V205e. CaForeattt part of iTIS qtestfoni; tonsider FOHOWIHg Btetat: You need to make a stock solution of Ca( C2H3O2 )2 with a concentration of 6.50 M. You have a 850.0 mL volumetric flask available to make this stock solution in. You are then tasked with using this stock solution to prepare a sample for use in an experiment. The experimental sample should have a final volume of 15.0 mL and a concentration of 0.350 M Ca(C2H3O2)2. a) What is the molar mass of Ca(C2H3O2)2? b) How many moles of the solute would be needed to create the stock solution using the volumetric flask available? c) How many grams of the solute should be added to the volumetric flask to create the stock solution? d) What volume, in mL, of the stock solution should be used to prepare the experimental solution through dilution? US 目 M2K MnO4 +6 HCI -> 5Clz+ZKCI + 2 Mnclz +8 HzU HOw moles of Clz are produced by 25.983 moles many assuming an excess of Hcl is present?
- Seashells are made up of mostly CaCO3 (100.09 g/mol) and a substance called chitin which contains C, H, O and N. To determine the percentage of CaCO3present in a seashell, gravimetric analysis is performed by dissolving a shell in acid followed by treatment with NaC2O4 (134 g/mol) to produce solid CaC2O4 (128.1 g/mol). If a 514 g seashell found in Ocean City, MD undergoes this analysis to produce 598 g of CaC2O4, what is the percentage of CaCO3 in the shell? Assume 100% yield for the reaction. Report your answer to the tenths place and do not include the % sign.A 0.879 g sample of a CaCl2·2H2O/K2C2O4·H2O solid salt mixture is dissolved in ~100mL of deionized water. The precipitate, after having been filtered and air-dried, has a mass of 0.284 g. The limiting reactant in the salt mixture was later determined to beCaCl2 ·2H2O. a.Write the ionic equation for the reaction. b.Write the net ionic equation for the reaction. c.How many moles and grams of CaCl2 ·2H2O reacted in the reaction mixture? d.How many moles and grams of the excess reactant, K 2C2O 4H2O, reacted in the mixture? e.How many grams of the K2C2O4·H2O in the salt mixture remain unreacted (inexcess)? f.What is the percent by mass of each salt in the mixture0.004 C8H7NO3, 15mL ethanol, 0.002mol NaBH4 was used. HCl was used to acidify. It was then extracted with ether. Then it was dried and a mass of 0.32g was obtained. What is the balanced equation of this synthesis, and what is the limiting reagent?
- Over time, as their free fatty acid (FFA) content increases,edible fats and oils become rancid. To measure rancidity, the fator oil is dissolved in ethanol, and any FFA present is titrated withKOH dissolved in ethanol. In a series of tests on olive oil, a stocksolution of 0.050 Methanolic KOH was prepared at 25C, storedat 0C, and then placed in a 100-mL buret to titrate any oleic acid[CH₃(CH₂)₇CH=CH(CH₂)₇COOH] present in the oil. Each offour 10.00-g samples of oil took several minutes to titrate: thefirst required 19.60 mL, the second 19.80 mL, and the third and fourth 20.00 mL of the ethanolic KOH.(a) What is the apparent acidity of each sample, in terms of mass% of oleic acid? (Note:As the ethanolic KOH warms in the bu-ret, its volume increases by a factor of 0.00104/C.)(b) Is the variation in acidity a random or systematic error? Ex-plain.(c) What is the actual acidity? How would you demonstrate this?What is the percent magnesium hydroxide, if a sample of magnesia magma weighing 5.2430g when dissolved in 25 mL of 0.9915 N H2SO4 required 9.85 mL of 1.4102 N NaOH to titrate the excess acid? Round to 2 decimal point; Answer should be with the correct unit.2 HyPOalaq) + 3 Mg(OH)2(ag) = Mga (P04/21s) + 6 H201 If 35.0 mL of 1.67 M HsP04 are reacted with 50.0 mL of 1.25 M Mg(OH)2 and 4.892 g of Mg(P042 (M. W. =262.86 g/mole) are collected: What species is the limiting reagent? the theoretical yield of Mg(P04) in grams? Whatis thr molarity of excess reagent left over in solution ?
- What mass of FeS is required to produce 87g Fe2O3 with excess O2 by this reaction 4FeS + 7 O2 —> 2Fe2O3 + 4SO2Secondly, each group should do the following Pre-calculations for preparing solutions during the laboratory (calculating weight and volume) for the following solutions: 1-Prepare the KOH solution: concentration= 1.4 M in 50 ml (= 0.05 L) Volumetric flask, M.wt = 56.11 g.mol-1, weight of KOH? 2- Prepare the H2SO4 solution: density = 1.84, % 98, M.wt 98.08. what the volume to prepare H2SO4 with 9 M (M2) in 50 ml (V2).A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.