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Analysis: 1. Reconcile your prediction with your observations. Write a definition for limiting and excess reactants based on your observations. 2. Calculate the number of moles of the excess reactant that is left over in each of the reaction trials: Trial 1: Trial 2: Trial 3: I

Analysis: 1. Reconcile your prediction with your observations. Write a definition for limiting and excess reactants based on your observations. 2. Calculate the number of moles of the excess reactant that is left over in each of the reaction trials: Trial 1: Trial 2: Trial 3: I

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter2: Chemical Formulas, Equations, And Reaction Yields
Section: Chapter Questions
Problem 38P: Titanium dioxide, TiO2 , reacts with carbon and chlorineto give gaseous TiCl4 :...
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es) 80 1. Measure 5 separate quantities of sodium hydrogen carbonate (NaHCO3) trying to get the five samples close to 0.5 g, 0.4 g, 0.3 g, 0.2 g and 0.1 g. Record the exact masses in table 2.1 2. Obtain about 40mL of the 0.7 M HCI in your 50mL beaker. 3. Add 2 drops of indicator to each flask, observe any color change. 4. Set up gas collection apparatus as demonstrated by TA 5. Collect 5.00 mL of hydrochloric acid into the syringe 6. Inject the acid and allow to react (make sure to think about how to account for this volume when measuring the volume of gas produced) Data: HCl(aq) + NaHCO3(s) → CO2(g) + H20(1) + NaCl(aq) Table 2.1 Flask 1 2 3 Results: Table 2.2 F4 Complete table 2.2 Flask 1 2 Q Volume of 0.700 MHCI (ml) 5.00 mL 5.00 mL 3 5.00 mL Color of Solution After Reaction Light pink pink Clear F5 Mole HCI Volume of gas produced 29 ml 68 ml 67 ml Solid ResidueY/N F6 N N Y Equation 2.1 Mass of NaHCO3 (g) 0.1 g 0.3 g 0.5 g What reactant was limiting, i.e. used up? NaHCO3 NaHCO3 HCI F7 Mole NaHCO3 (84.0 g/mol) What reactant was in excess, i.e.some left over? HCI HCI NaHCO3 DII F8 Focus F9
Transcribed Image Text:es) 80 1. Measure 5 separate quantities of sodium hydrogen carbonate (NaHCO3) trying to get the five samples close to 0.5 g, 0.4 g, 0.3 g, 0.2 g and 0.1 g. Record the exact masses in table 2.1 2. Obtain about 40mL of the 0.7 M HCI in your 50mL beaker. 3. Add 2 drops of indicator to each flask, observe any color change. 4. Set up gas collection apparatus as demonstrated by TA 5. Collect 5.00 mL of hydrochloric acid into the syringe 6. Inject the acid and allow to react (make sure to think about how to account for this volume when measuring the volume of gas produced) Data: HCl(aq) + NaHCO3(s) → CO2(g) + H20(1) + NaCl(aq) Table 2.1 Flask 1 2 3 Results: Table 2.2 F4 Complete table 2.2 Flask 1 2 Q Volume of 0.700 MHCI (ml) 5.00 mL 5.00 mL 3 5.00 mL Color of Solution After Reaction Light pink pink Clear F5 Mole HCI Volume of gas produced 29 ml 68 ml 67 ml Solid ResidueY/N F6 N N Y Equation 2.1 Mass of NaHCO3 (g) 0.1 g 0.3 g 0.5 g What reactant was limiting, i.e. used up? NaHCO3 NaHCO3 HCI F7 Mole NaHCO3 (84.0 g/mol) What reactant was in excess, i.e.some left over? HCI HCI NaHCO3 DII F8 Focus F9
Analysis: 1. Reconcile your prediction with your observations. Write a definition for limiting and excess reactants based on your observations. 2. Calculate the number of moles of the excess reactant that is left over in each of the reaction trials: Trial 1: Trial 2: Trial 3: I
Transcribed Image Text:Analysis: 1. Reconcile your prediction with your observations. Write a definition for limiting and excess reactants based on your observations. 2. Calculate the number of moles of the excess reactant that is left over in each of the reaction trials: Trial 1: Trial 2: Trial 3: I
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