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Chelsea Fenderson 6/10/20 Stoichiometry by Loss of CO2_MC1_Mass of Flask 1

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Chelsea Fenderson

6/10/20

Stoichiometry by Loss of CO2_MC1_Mass of Flask

1.         What was the mass of the empty Erlenmeyer flask?

            A.        116.615 g                                                        B.        110.615 g

            C.        110.000 g                                                        D.        94.000 g

Stoichiometry by Loss of CO2_MC2_Flask and Sulfuric Acid Mass

2.         What was the mass of the flask plus sulfuric acid? Choose the closest answer.

            A.        117.934 g                                                        B.        94.000 g

            C.        110.000 g                                                        D.        20.000 g

Stoichiometry by Loss of CO2_MC3_Mass of Flask 1 After Reaction

3.         What was the mass of flask 1 after the reaction? Choose the closest answer.

            A.        112.955 g                                                        B.        111.615 g

            C.        110.615 g                                                        D.        118.519 g

 

 

Stoichiometry by Loss of CO2_MC4_Mass of Flask 5 After Reaction

4.         What was the mass of flask 5 after the reaction? Choose the closest answer.

            A.        112.955 g                                                        B.        123.293 g

            C.        110.615 g                                                        D.        119.975 g

Stoichiometry by Loss of CO2_MC5_Mass of Carbon Dioxide Generated

5.         How much carbon dioxide was generated in flask 1 after adding sodium carbonate? Choose the closest answer.

            A.        0.585 g            B.        1.200 g            C.        0.415 g            D.        111.200 g

Stoichiometry by Loss of CO2_MC6_Contents of Flask

6.         What happened to the contents of the flask after adding sodium carbonate to the sulfuric acid?

            A.        Nothing happened.

            B.        They increased in volume as water was absorbed by the system.

            C.        They turned grey as a precipitate formed.

            D.        They bubbled as gas was released.

Stoichiometry by Loss of CO2_MC7_Moles Sodium Carbonate Added

7.         How many moles of sodium carbonate were added to flask 1? The molar mass of sodium carbonate is 105.99 g/mol.

            A.        0.06000 mol                                                    B.        0.009435 mol

            C.        0.01887 mol                                                    D.        1.000 mol

Stoichiometry by Loss of CO2_MC8_Moles CO2 Released in Flask 1

8.         How many moles of carbon dioxide were released from the reaction in flask 1? The molar mass of carbon dioxide is 44.01 g/mol.

            A.        0.0600 mol                                                      B.        0.415 mol

            C.        0.00943 mol                                                    D.        0.0289 mol

 

Stoichiometry by Loss of CO2_MC9_Moles CO2 Released in Flask 5

9.         How many moles of carbon dioxide were released from the reaction in flask 5? The molar mass of carbon dioxide is 44.01 g/mol.

            A.        0.0600 mol                                                      B.        2.64 mol

            C.        0.0289 mol                                                      D.        0.0755 mol

Stoichiometry by Loss of CO2_MC10_Moles H2SO4 Used

10.       How many moles of sulfuric acid were used in this experiment?

            A.        20.0 mol                                              B.        0.0600 mol

            C.        0.150 mol                                            D.        6.67 mol

Stoichiometry by Loss of CO2_MC11_Limiting Reactant in Flask 1

11.       What was the limiting reactant in flask 1?

            A.        carbon dioxide                                                B.        water

            C.        sodium carbonate                                D.        sulfuric acid

Stoichiometry by Loss of CO2_MC12_Limiting Reactant in Flask 5

12.       What was the limiting reactant in flask 5?

            A.        water                                                   B.        carbon dioxide

            C.        sodium carbonate                                D.        sulfuric acid

Stoichiometry by Loss of CO2_MC13_Ratio Between Sodium Carbonate and Carbon Dioxide

13.       What is the stoichiometric ratio between sodium carbonate and carbon dioxide?

            A.        1:2                   B.        3:2                   C.        1:1                   D.        2:1

 

 

 

Stoichiometry by Loss of CO2_MC14_Analyze Graph

14.       Below is a graph of the number of moles of CO₂ produced as a function of the number of moles of Na₂CO₃ added. How does the graph appear?

 

 

A.        The number of moles of CO₂ increases linearly with increasing Na₂CO₃ until around 0.06 moles of Na₂CO₃, at which point, the amount of CO₂ produced is independent of the amount of Na₂CO₃ added.

B.        The number of moles of CO₂ gas produced increases with increasing Na₂CO₃ over the range of all concentrations of Na₂CO₃ added.

C.        There is not enough information to determine this relationship.

D.        The number of moles of CO₂ gas produced is independent of the amount of Na₂CO₃ added because it only depends on the amount of sulfuric acid.

Stoichiometry by Loss of CO2_MC15_Determine Why Bubbles Appear in Reaction

15.       Why did the solution bubble when the Na₂CO₃ was added?

            A.        The H₂SO₄ in solution underwent a phase transition.

            B.        Bubbles did not form.

            C.        CO₂ gas was produced.

            D.        Na₂CO₃ gas was produced.