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5) Discuss the sources of error in your experiment. 6) List three practical applications of MgO and o.

5) Discuss the sources of error in your experiment. 6) List three practical applications of MgO and o.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
Problem 118QRT
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I just want to make sure if my work is correct. I also need help answering questions 5 and 6 on the last page. Please and thank you.

Gerardo Benitez Chemistry 1A Name Lab Partner Hector Part 2C: Heat of Formation of Metal oxide (Enthalpy of formation of metal oxide) 1) Write the balanced equation for the heat of formation of magnesium oxide and zine oxide. Ma (s)+ Ź O2 (9) Mg O (s) 2) Using Hess's Law, determine the enthalpy of formation of both the metal oxides, MgO and ZnO. To do this, you will need the balanced thermochemical equations for the two reactions studicd in this lab, plus the balanced thermochemical equation for the formation of water from its clements. Clearly show below how these three equations (and their reaction enthalpies) must be combined to give the target reaction for enthalpy of formation of both the metal oxides. (For the metal/ metal oxide that was not assigned to you, take the data for AHn from students on your bench) Enthalpy of formation of MgO: (Show equations and calculations below) Mg(3)サ 2HC1(ag)→ (aq) + H2 9) (a2) t My Orso AH3=-285,9 ks/mc Mg (s)+ b Oz(9) + Mg Ors) Enthalpy of formation of ZnO: (Show equations and calculations below) Experiment 3-Thermochemistry-Calorimetry and Hess's Law Page 8 of 12
Transcribed Image Text:Gerardo Benitez Chemistry 1A Name Lab Partner Hector Part 2C: Heat of Formation of Metal oxide (Enthalpy of formation of metal oxide) 1) Write the balanced equation for the heat of formation of magnesium oxide and zine oxide. Ma (s)+ Ź O2 (9) Mg O (s) 2) Using Hess's Law, determine the enthalpy of formation of both the metal oxides, MgO and ZnO. To do this, you will need the balanced thermochemical equations for the two reactions studicd in this lab, plus the balanced thermochemical equation for the formation of water from its clements. Clearly show below how these three equations (and their reaction enthalpies) must be combined to give the target reaction for enthalpy of formation of both the metal oxides. (For the metal/ metal oxide that was not assigned to you, take the data for AHn from students on your bench) Enthalpy of formation of MgO: (Show equations and calculations below) Mg(3)サ 2HC1(ag)→ (aq) + H2 9) (a2) t My Orso AH3=-285,9 ks/mc Mg (s)+ b Oz(9) + Mg Ors) Enthalpy of formation of ZnO: (Show equations and calculations below) Experiment 3-Thermochemistry-Calorimetry and Hess's Law Page 8 of 12
Name_Gerade Benidez Chemistry 1A Lab PartnerHector 3) Write the AH value for the metal oxides from the table in the textbook. -C01.8 Ko/mol MgO: 4) Determine the percent error in the experimentally determined value for the enthalpy of formation of both metal oxides. Theor Exp.! f erfor- x100= Theo Xl00 = -23. 56 % -601.8 -2 36% 5) Discuss the sources of error in your experiment. 6) List three practical applications of MgO and Z0. Experiment 3-Thermochemistry-Calorimetry and Hess's Law Page 9 of 12
Transcribed Image Text:Name_Gerade Benidez Chemistry 1A Lab PartnerHector 3) Write the AH value for the metal oxides from the table in the textbook. -C01.8 Ko/mol MgO: 4) Determine the percent error in the experimentally determined value for the enthalpy of formation of both metal oxides. Theor Exp.! f erfor- x100= Theo Xl00 = -23. 56 % -601.8 -2 36% 5) Discuss the sources of error in your experiment. 6) List three practical applications of MgO and Z0. Experiment 3-Thermochemistry-Calorimetry and Hess's Law Page 9 of 12
Expert Solution
Step 1

1,2,3 and 4 is correct.

5. Sources of error 

a. At the time of measuring weight , fault in digital device.

b. Spilling of salt and liquid.

c. Leak in CALORIMETER.

d. Not stirring solution too well.

e. Incorrect reading of thermometer.

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