2) 3. H₂O, heat HO

The 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

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Write a balanced equation for the Alka Seltzer reaction where aqueous citric acid, H3C6H5O7, and aqueous sodium bicarbonate, NaHCO3, react and form aqueous sodium citrate, liquid water, and carbon dioxide gas.

Mesitylene is a liquid hydrocarbon. Burning 0.795 g of the compound in oxygen gives 2.62 g of CO2 and 0.716 g of H2O. What is the empirical formula of mesitylene?

2.) 350 g of Calcium Chromate reacts with excess Hydrogen Peroxide. Write a balanced chemical equation and then calculate what mass of Calcium Peroxide will be formed.

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).

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?