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Compare the value you calculated with the actual value (-601.8 kJ/mol). Show your determination of percent error. Use the standard equation for this: actual value - experimental value %error = x 100% |actual value|

Compare the value you calculated with the actual value (-601.8 kJ/mol). Show your determination of percent error. Use the standard equation for this: actual value - experimental value %error = x 100% |actual value|

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter9: Chemical Quantities
Section: Chapter Questions
Problem 75AP
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2. Compare the value you calculated with the actual value (-601.8 kJ/mol). Show your determination of percent error. Use the standard equation for this: actual value - experimental value %error = x 100% |actual value| ragraph* and which the & 3 4 7 8
Transcribed Image Text:2. Compare the value you calculated with the actual value (-601.8 kJ/mol). Show your determination of percent error. Use the standard equation for this: actual value - experimental value %error = x 100% |actual value| ragraph* and which the & 3 4 7 8
Room Temperature Reactant Mg Mg MgO MgO Trial Number 1 2 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 (ti) (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 (T?) (calculate from linear fit data) 37.31 44.71 34.57 39.14 AT =Tr-Ti 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 qrxn -5616.324 J -5530.644 J -1657.908 J -1687.896 J 598.321 KJ/ 528.237 KJ/ mol 120.954 KJ/ mol 129.838 KJ/ mol ΔΗ 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 (1) AH = (calculated in the experiment) H2 (g) + ½02 (g) → H20 (1) AH=- 285.8 kJ/mol Mg (s) + ½ 02 (g) → Mg0 (s) AH = (determine using Hess's Law) st Paragraph* and which the
Transcribed Image Text:Room Temperature Reactant Mg Mg MgO MgO Trial Number 1 2 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 (ti) (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 (T?) (calculate from linear fit data) 37.31 44.71 34.57 39.14 AT =Tr-Ti 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 qrxn -5616.324 J -5530.644 J -1657.908 J -1687.896 J 598.321 KJ/ 528.237 KJ/ mol 120.954 KJ/ mol 129.838 KJ/ mol ΔΗ 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 (1) AH = (calculated in the experiment) H2 (g) + ½02 (g) → H20 (1) AH=- 285.8 kJ/mol Mg (s) + ½ 02 (g) → Mg0 (s) AH = (determine using Hess's Law) st Paragraph* and which the
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