Worksheet # 6 Quarter 3 Packet 6
					Name:  _________________________
		Atomic Stoichiometry Mr. Schuett adds 217g of iron(111) carbonate to a beaker containing HCl. 1.  Write out the balance chemical reaction. 2.  Calculate the mass of iron(111) chloride and the mass of water that are produced in the reaction 3.  Mr. Schuett wants to fill a large ballon with the carbon dioxide that is produced by this reaction.  What mass of hydrochloric acid will he have to use in order to produce a volume of 100. L of CO2 at STP? 4. How many molecules of iron(111) carbonate does Mr. Schuett need to react with 5.0 x 10^25 formula units of HCl?  What is the mass of this quantity of iron(111) carbonate?
	Mr. Schuett dissolved 2.05 g of copper(11) sulfate pentahydrate in water.  He then added 24.0 g of NaOH to the solution and gently heated it to boiling.  This reaction produced Cu(OH)2, which he filtered out of the solution.  The solid was then dried to break it down into copper(11)oxide and water Note: A hydrate is a compound that contains a salt and water combined in definite proportions.  Frequently, when water is evaporated from an aqueous salt solution a certain number of water molecules remain in the resulting solid but still retain their chemical identity.  The dot  in the formula for a hydrate indicates that the salt and water molecules are closely associtated with each other in a constant ratio but each type of molecule is chemically distinct. The steps in this reaction are listed below: 1. CuSO4 (dot) 5H2O(s) (yields) CuSo4 + 5H2O 2. CuSO4 + 2NaOH (yields) Cu(OH)2(s) + Na2SO4 3. Cu(OH)2 (yields) CuO(s) + H2O Questions 1.  Fill in each blank with the correct answer. Reaction Step  Mass of          Mass of Copper  Percent Yield                       Reactant (g)    Product (g) 1                   2.05                (       )                 100%           2                   (     )               (       )                 100% 3                   (     )               (       )                 100%