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 12.5g of CaCO3 and 17.3g 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 MIntroduce the excess NH3 through a 600g solution of 42% HNO3 and taking out 300 g ammonium nitrate. Determine the yield of ammonium nitrate.
- 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.Select the coefficients needed to balance this equation. KClO3 --> KCl + O22K 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?
- Answers accurate to 3 or 4 significant figures & show your work. 5. The dichromate ion, Cr2072- reacts with methanol, CH3OH in acidic solution according to the equation below. If 200.0 mL of 1.00 M Cr2O7?-(aq) reacts with 200.0 mL of 1.875 M CH3OH (aq) in the presence of 200.0 mL of 10.0 M H† (aq), show how you determine (a) the limiting reagent and moles of each of the two excess reagents left at the end of the reaction [Hint: H* is one of the excess reagents!]; (b) the number of moles & grams of all products expected to form; and (c) the molar concentration of each type of aqueous species present in the final mixture. The balanced chemical equation is 2 Cr207 (aq) + 3 CH3OH (aq) + 16 H*(aq) → 4 Cr*(aq) + 3 HCO2H (aq) + 11 H2O (1)A popular brand of tea powder contains 3.5% caffeine as indicated by the label on it. 1.80 g of the tea powder was used to extract caffeine from it and obtained 0.031 g of pure caffeine. What is the percentage recovery of caffeine based on the caffeine content (as labeled) in the tea powder? O 49.21% O 1.72% O 62.50% O 42.25%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 mixture
- The number of moles of H2O produced in reaction of 50 mL 1.0 M CH3COOH and 50 mL 1.0 M NaOH.What volume (mL) of 0.0665 M KMnO4 is necessary to convert 12.5 g KI (166.00 g/mol) to I2 in the reaction [2KMnO4 + 10KI + 8H2SO4 ( 6K2SO4 + 2MnSO4 + 5I2 + 8H2O]. Assume that H2SO4 is present in excess.The first goal is to make the oxalic acid standard solution. You measure 1.5232 g of oxalic acid on an analytical balance, add it to a 250-mL volumetric flask and add deionized H2O to a final volume of 250.0 mL. Molar mass of H2C2O4•2H2O = 126.07 g/mol Mass of H2C2O4•2H2O = 1.5232g Volume of H2C2O4•2H2O solution = 250.0mL What is the Molarity H2C2O4 standard solution ?