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- 3.122 What type of reasoning were we using when we developed the equation for dilution, MiVi=MfVf ?Tungsten (W) metal, which is used to make incandescent bulb filaments, is produced by the reaction WO3+3H23H2O+W How many grams of H2 are needed to produce 1.00 g of W?4. A hydrate of iron (II) sulphate, FESO, xHI,0 is 20.0% iron by mass. A) What is the chemical formula for the hydrated compound? B) During this lab experiment, "splattering" of the hydrate is a common source of error. Splattering occurs when heat gets trapped under the salt and pops ejecting some of the hydrate from the beaker. Explain how splattering will affect the ratio of the anhydrous salt to water.
- 6.) Hydrogen peroxide H2O2 is commonly used to clean bacteria in scrapes and cuts. It can be used as a mouthwash and is an additive in some toothpastes. If a sample contained 5.23 x 1021 molecules of H2O2 what would the equivalent be in moles? A) 8.69 x 10-3 mol B) 8.69 x 103 mol C) 115 mol D) 8.69 x 1043 molThe semi-precious stone turquoise is a hydrate and with the chemical formula CuAls(PO4)-(OH);·4 H2O. a) How many aluminum atoms are in one formula unit of the hydrate? b) How many oxygen atoms are in one formula unit of the hydrate? c) What is the molar mass of the hydrate? d) What is the mass percent of aluminum in the hydrate? e) What is the mass percent of oxygen in the hydrate? f) What is the mass percent of water in the hydrate?1. Explain the term empirical formula and a molecular formula and state how they two differ. 2. Write the empirical formulas of the following: (a) H₂O₂= ; (b) C¿H= ; (c) C6H₁2O6 = ; (d) H₂0 = (e) MgO 12 NaOH g of O 3. Calculate the formula mass (a) NaCl = (b) KOH of Cu 9 = 4. What is the percentage of Ag in AgNO3 5. What is the percentage of C in C12H22O11 (Sucrose, Cane Sugar) 6. Determine in g the mass of 2.5 moles of = 7. How many moles in 0.5 g of Mg; and 0.2 of C₂H₂O₂. ; 8. Determine the number of atoms in 0.8 g 9. A substance was found by analysis to contain 45.57 % of Sn and 54.43 % of Cl. What is the empirical formula of the substance. 10. Ethylene Glycol has a molecular formula (a) Determine its molar mass (b) The percentage compositions of its component's elements (c) The empirical formula of Ethylene Glycol
- 1. What is the mass percentage composition of capsaicin? 2. What is the percentage composition of sodium in baking soda, a component of some anti-acid tablets sold over the world?4. Write a balanced equation for the combustion of liquid methyl alcohol (CH3OH) in the presence of oxygen (O2), to produce carbon dioxide gas and gaseous water (dihydrogen oxide).1. CFC s are compounds that contain only carbon, chlorine and fluorine. They are atmospheric pollutants and destroy ozone in the upper atmosphere. a) CFC 11 has the following composition by mass: C – 8.7 % ; F -13.8 %; Cl – 77.5 % Calculate the empirical formula of CFC11. b) CFC 12 has the molecular formula CF2Cl2. It can be made by the reaction of hydrogen fluoride , HF with tetrachloromethane, CCl4.. CCl4 + 2HF → CCl2F2 + 2HCl. What is the maximum mass of CFC 12 that can be made from 10.0 g of hydrogen fluoride?
- 2.Iron ore is impure Fe2O3. When Fe2O3 is heated with an excess of carbon (coke), metallic iron and carbon monoxide gas are produced. From a sample of ore weighing 938 kg, 523 kg of pure iron is obtained. What is the mass percent Fe2O3 by mass, in the ore sample, assuming that none of the impurities contain Fe?Bromine (Br) and Silver has atomic masses of 79.90 g and 107.9 g. respectively. In a certain experiment, a sample of 0.3320 g of an ionic compound containing the bromide ion (Br-) is dissolved in water and treated with an excess of AgNO3. The mass of AgBr precipitate that forms is 0.734 g. Br = 79.90 amu; Ag = 107.9 amu 1. Determine the percent Br in Ag Br. Answer in 2 decinal places. 2. Determine the mass of Br in 0.734 g AgBr. Answer in 4 decimal places. 3. Calculate the percent by mass of Br in the original compound. Answer in 2 decimal places.6. Çalculate the mass (in g) of 2.3 x 1021 molecules of CO2.
