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Use the following to determine the enthalpy of formation of magnesium oxide: Mg (s) + 2HCI (aq) →MgCl2 (aq) + H2 (g) AH=(calculated in the experiment) Mg0 (s) + 2HCI (aq) → MgCl2 (aq)+ H2O (1) AH=(calculated in the experiment) H2 (g) + ½02 (g)→ H20 (1) AH=-285.8 kJ/mol Mg (s) + ½ O2 (g) → Mg0 (s) AH=(determine using Hess's Law) Calculations: 1. Using the enthalpies of reaction computed in the lab and the value given for the enthalpy of formation of liquid water, show the Hess's Law determination of the enthalpy of formation of solid magnesium oxide!

Use the following to determine the enthalpy of formation of magnesium oxide: Mg (s) + 2HCI (aq) →MgCl2 (aq) + H2 (g) AH=(calculated in the experiment) Mg0 (s) + 2HCI (aq) → MgCl2 (aq)+ H2O (1) AH=(calculated in the experiment) H2 (g) + ½02 (g)→ H20 (1) AH=-285.8 kJ/mol Mg (s) + ½ O2 (g) → Mg0 (s) AH=(determine using Hess's Law) Calculations: 1. Using the enthalpies of reaction computed in the lab and the value given for the enthalpy of formation of liquid water, show the Hess's Law determination of the enthalpy of formation of solid magnesium oxide!

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Use the following to determine the enthalpy of formation of magnesium oxide: Mg (s) + 2HCI (aq) →MgCl2 (aq) + H2 (g) AH=(calculated in the experiment) Mg0 (s) + 2HCI (aq) → MgCl2 (aq)+ H2O (1) AH=(calculated in the experiment) H2 (g) + ½02 (g)→ H20 (1) AH=- 285.8 kJ/mol Mg (s) + ½ O2 (g) → Mg0 (s) AH=(determine using Hess's Law) Calculations: 1. Using the enthalpies of reaction computed in the lab and the value given for the enthalpy of formation of liquid water, show the Hess's Law determination of the enthalpy of formation of solid magnesium oxide. List Paragraph* West Hello
Transcribed Image Text:Use the following to determine the enthalpy of formation of magnesium oxide: Mg (s) + 2HCI (aq) →MgCl2 (aq) + H2 (g) AH=(calculated in the experiment) Mg0 (s) + 2HCI (aq) → MgCl2 (aq)+ H2O (1) AH=(calculated in the experiment) H2 (g) + ½02 (g)→ H20 (1) AH=- 285.8 kJ/mol Mg (s) + ½ O2 (g) → Mg0 (s) AH=(determine using Hess's Law) Calculations: 1. Using the enthalpies of reaction computed in the lab and the value given for the enthalpy of formation of liquid water, show the Hess's Law determination of the enthalpy of formation of solid magnesium oxide. List Paragraph* West Hello
Room Temperature Reactant Mg Mg MgO MgO Trial Number 3 4 Mass of reactant (from data) 0.2529 g 0.2545 g 0.552g 0.5241 g Moles of reactant (calculate) 0.01041 0.01047 0.0137 0.0130 Initial time (t) (from graph) 18.0 sec 16.0 sec 30.5 sec 28.5 sec Initial Temperature (Ti) (from the graph) 24.2 31.8 30.7 35.2 Linear Curve fit slope (m) (from the graph) -0.00655 -0.009704 -0.004660 -0.00858 Linear Curve fit intercept (b) (from the graph) 37.31 44.71 34.57 39.14 Final Temperature (Tr) (calculate from linear fit data) 37.31 44.71 34.57 39.14 AT = Tr-T¡ 13.11 12.91 3.87 3.94 qwater 13.11 12.91 3.87 3.94 qcalorimeter 131.1 J 129.1 J 38.7 J 39.4 J qrın -5616.324 J -5530.644 J -1657.908 J -1687.896 J 598.321 KJ/ mol 528.237 KJ/ mol 120.954 KJ/ mol 129.838 KJ/ AHrxn mol Use the following to determine the enthalpy of formation of magnesium oxide: Mg (s) + 2HCI (aq) → MgCl2 (aq) + H2 (g) AH=(calculated in the experiment) Mg0 (s) + 2HCI (aq) → MgCl2 (aq)+ H20 (I) AH=(calculated in the experiment) H2 (g) + ½02 (g) → H20 (1) AH =- 285,8 kJ/mol Paragraph* West Hello
Transcribed Image Text:Room Temperature Reactant Mg Mg MgO MgO Trial Number 3 4 Mass of reactant (from data) 0.2529 g 0.2545 g 0.552g 0.5241 g Moles of reactant (calculate) 0.01041 0.01047 0.0137 0.0130 Initial time (t) (from graph) 18.0 sec 16.0 sec 30.5 sec 28.5 sec Initial Temperature (Ti) (from the graph) 24.2 31.8 30.7 35.2 Linear Curve fit slope (m) (from the graph) -0.00655 -0.009704 -0.004660 -0.00858 Linear Curve fit intercept (b) (from the graph) 37.31 44.71 34.57 39.14 Final Temperature (Tr) (calculate from linear fit data) 37.31 44.71 34.57 39.14 AT = Tr-T¡ 13.11 12.91 3.87 3.94 qwater 13.11 12.91 3.87 3.94 qcalorimeter 131.1 J 129.1 J 38.7 J 39.4 J qrın -5616.324 J -5530.644 J -1657.908 J -1687.896 J 598.321 KJ/ mol 528.237 KJ/ mol 120.954 KJ/ mol 129.838 KJ/ AHrxn mol Use the following to determine the enthalpy of formation of magnesium oxide: Mg (s) + 2HCI (aq) → MgCl2 (aq) + H2 (g) AH=(calculated in the experiment) Mg0 (s) + 2HCI (aq) → MgCl2 (aq)+ H20 (I) AH=(calculated in the experiment) H2 (g) + ½02 (g) → H20 (1) AH =- 285,8 kJ/mol Paragraph* West Hello
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