Write a balanced equation for the following by inserting the correct coefficients. If the coefficient equals 1, add "1" in the provided box. CaSiO3(s) + HFg)- SiF (g) + CaF2(s) + H2O(1)
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- Balance the equation by inserting coefficients as needed. ___C2H6O+____O2⟶___CO2+____H2OStock 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.balance C6H12O6+CO2+H2O with explanation
- Show your work: Balance the following chemical equation: C7H16O5 + O2 ---> CO2 + H2OUsing the percent purity calculations, determine the percent yield of synthesis of aspirin. Part I Synthesis of Aspirin Mass of salicylic acid used (g) 2.029g Volume of acetic anhydride used (mL) 5ml Mass of acetic anhydride used (vol. × 1.08 g/mL) 5.4g Mass of aspirin synthesized (g) 3.256g Part II Melting Temperature Data Melting temperature (°C) 133°C Part III Salicylic Acid Standard Stock Solution Initial mass of salicylic acid (g) 0.210g Moles of salicylic acid (mol) 0.0147 mol Initial molarity of salicylic acid (M) 0.724 M Part III Beer’s Law Data for Salicylic Acid Standard Solutions Trial Concentration (M) Absorbance Water (mL) 1 10 0.301 0 2 7.5 0.219 2.5 3 5.0 0.163 5.0 4 2.5 0.074 7.5 Best-fit line equation for the salicylic acid standards Test of the Purity of the Synthesized Aspirin Initial mass of aliquot of product (g)…Pure CO2 may be prepared by treating limestone with sulfuric acid. The limestone used in the process contains CaCO3, MgCO3 and inert. The acid used contains 12% H2SO4 by weight The residue from the process had the following composition. CaSO4 – 8.56%; MgSO4 – 5.23%; H2SO4 – 1.05%; Inert – 0.53%; CO2 – 0.12%; H2O – 84.51%; During the process, the mass was warmed where CO2 and H2O were removed. Calculate the following.a) The analysis of lime stone and b) The % excess acid used.
- Using the data collected (e.g., masses of hydrated metal salt and oxalic acid 1M reacted and actual yield of hydrated metal oxalate precipitate) and the balanced reaction for the formation of the metal oxalate product determine: 4.031g of ammonium iron (II) sulfate hexahydrate concentration of oxalic acid : 50mL of 1M oxalic acid ferrous oxalate dihydrate was formed weighed (Actual Yield) 1.746g. 1. identity of the limiting reactant in the synthesis of ferrous oxalate, 2.Theoretical yield of the ferrous oxalate dihydrate complex, and 3.The per cent yield of the ferrous oxalate dihydrate product of this reaction.Balance the following equation by selecting the coefficients in the dropdown boxes.The coefficient for C5H12 isa. 1b. 2c. 3d. 4The coefficient for O2 isa. 1b. 2c. 3d. 4e. 5f. 6g. 7h. 8i. 9j. 10The coefficient for CO2 is a. 1b. 2c. 3d. 4e. 5f. 6g. 7h. 8i. 9j. 10The coefficient for H2O is a. 1b. 2c. 3d. 4e. 5f. 6g. 7h. 8i. 9j. 10Zinc and magnesium react with hydrochloric acid to produce the metal chlorides and hydrogen gas. A 10.00 gram smaple of a mixture of Zn and Mg was with the stoichiometric quanitity of HCl. The reaction mixture was then reacted with 156 mL of 3.00M silver nitrate to produce the maximum quantity of silver chloride. First determine the % magnesium in the mixture- then, if 76.0 mL of HCl was added, what was the molarity of the HCl?