Name (First and Last): Stoichiometry and Mass Relationships Report Pages Obtain values from the pictures found in the procedure to complete the data table below A. Data: 65.62 + Mass beaker + NaCO3 + 66.62g 65.62g 2 Mass empty beaker 3 Mass Na:COs used 19. 4 Mass graduated cylinder + HCl(aq) 5 Mass empty graduated cylinder 12.689 4.41 g 8. 279 1 74.899 Mass HCl(aq) used 65.629 19 8.27 Total mass before rxn: beaker + Nazco, + HCl(aq) 65.623 8 Mass beaker + salt solution after reaction 74.469 9 Mass of CO2 generated by reaction Mass of beaker + NaCl (after drying) 66.729 B. Calculations and Questions 1. Write a balanced equation for the reaction between sodium carbonate (Na2CO3) and hydrochloric acid (HCI). 1 | Page

Name (First and Last): 2. Calculate the theoretical yield of the gas (CO2) that should be produced from the mass of Na2COused. Use dimensional analysis. 3. Use the following equation to calculate the percent yield of the CO2 in your experiment %yield = experimental (actual) theoretical (calculated) d elet 4. Calculate the theoretical yield of the salt (NaCl) that should be produced from the mass of Na2CO3 used. Use dimensional analysis. 5. Use the following equation to calculate the percent yield of the NaCl in your experiment. %yield = experimental (actual) x 100 theoretical (calculated) 6 Page

Name (First and Last): Practice problems: 1. Balance the following equations: a) KBr + Fe(OH)3 → __ KOH + __ FeBry KOH + __ Co(POc)2 → __ K3PO4 + — Co(OH)2 2. Write the balanced chemical equation for the production of bromine pentafluoride from liquid bromine and fluorine gas. Be sure to include physical states. 3. Write the balance chemical equation to show the formation of aqueous aluminum chloride and hydrogen gas upon reacting powdered aluminum with a solution of hydrochloric acid. Be sure to include physical states.

Name (First and Last): 4. Balance the following equation: NaOH + – H2SO4 → – H2O + Na2SO4 How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and you have an excess of sulfuric acid? 5. In a particular reaction 6.80g of dinitrogen trioxide gas (N203) was actually produced by reacting 8.75g of oxygen gas (O2) with excess nitrogen gas (N2). a) Write a balanced chemical equation for the reaction. Be sure to include physical states in the equation. b) Calculate the theoretical yield (in grams) of dinitrogen trioxide: Use dimensional analysis. c) Calculate the % yield of the product 8 Page