Question

Problem Set 7 Stoichiometry Calculations Name: Date: Lab Section: General Instructions: Complete the following problems, Circle answers and show all work on separate sheet(s) of paper. 5 problems will be chosen randomly for assessing a score on this assignment. Assignment is due at the end of the lab period. 1.) 5.0 g of magnesium metal is burned in excess oxygen to produce magnesium oxide. (a) Write a balanced chemical equation for this reaction with the correct phases of all substances shown. (b) How many grams of magnesium oxide are expected from this process? (e) How many moles of oxygen (0.) are required to completely consume the 5.0 grams of magnesium? (d) What type of reaction is this? 2.) Sulfuric acid is easily neutralized by potassium hydroxide to form water and a soluble salt. (a) Write a balanced chemical equation for this reaction with the correct phases of all substances shown. (b) If 3.5 mol of sulfuric acid are just neutralized, how many moles of potassium hydroxide are required? (c) If the reaction produces 15.0 g of water, how many grams of the salt will be produced? (d) Write the net ionic equation for this process 3.) Solution of lithium chloride and lead(II) acetate are mixed stoichiometrically. (a) Write a balanced chemical equation for this reaction with the correct phases of all substances shown. (b) Write the net ionic equation for this process. If no reaction indicate with "NR" in place of products. (c) If 0.250 g of lithium chloride is consumed, how many grams of lead II) acetate will be required? (d) If 0.250 g of lithium chloride is consumed with excess lead(II) acetate, how many grams of precipitate will be formed? 4.) Sodium sulfite reacts with hydrochloric acid to form water, a salt, and a gas. (a) Write a balanced chemical equation for this reaction with the correct phases of all substances shown. (b) How many moles of gas are formed if 2.0 mol of sodium sulfite is consumed in excess hydrochloric acid? (c) How many moles of hydrochloric acid are required to produce 10.0 g of the gaseous product? (d) Write the net ionic equation for this process. 5.) Magnesium carbonate can be decomposed upon heating to form carbon dioxide gas and magnesium oxide. (a) Write a balanced chemical equation for this reaction with the correct phases of all substances shown. (b) How many grams of the gas are produced if 2.5 g of magnesium carbonate are decomposed? (c) How many moles of magnesium carbonate would be required to produce 2.5 g of the gas? (d) What type of reaction is this? 6.) The Thermite reaction involves combining ferric oxide and aluminum metal and produces great quantities of heat. (Note: "ferric" is the Feion) (a) Write a balanced chemical equation for this reaction with the correct phases of all substances shown. (b) If 5.0 g of aluminum are consumed, how many grams of the metallic product are formed? (c) If you wanted to make 5.0 g of the metallic product, how many moles of ferric oxide would be required? (d) What type freaction is this? 7.) Given: 5,0 g sodium metal is added to 10.0 g of water to produce a basic salt and a gas. (a) Write a balanced chemical equation for this reaction with the correct phases of all substances shown. (b) Which substance is the limiting reagent under these conditions? Show with calculation(s)? (c) What is the theoretical yield (in grams) of the gaseous product? (d) What is the theoretical yield (in grams) of the aqueous product? 80

Answer 1

Answer to first question is attached

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