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Room Temperature Reactant Trial Number Mass of reactant (from data) 26.0°C Mg 1 0.2578 g Mg 2 0.2551 g MgO 3 0.4939 g MgO 4 0.5033 g

Room Temperature Reactant Trial Number Mass of reactant (from data) 26.0°C Mg 1 0.2578 g Mg 2 0.2551 g MgO 3 0.4939 g MgO 4 0.5033 g

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Water mass 100.0 mL of pure water. 

heat capacity of the calorimeter as 10.0 J/ºC

Room Temperature Reactant Trial Number Mass of reactant (from data) Moles of reactant (calculate) Initial time (ti) (from graph) Initial Temperature (Ti) (from the graph) Linear Curve fit slope (m) (from the graph) Linear Curve fit intercept (b) (from the graph) Final Temperature (T) (calculate from linear fit data) AT = T₁-Ti qwater calorimeter qrxu AHrxn 26.0°C Mg (s) + O2 (g) → MgO (s) Mg 1 0.2578 g 33.5 s 24.3°C Mg 37.23 °C 2 0.2551 g 41.05 s 29.055 °C MgO 41.72 °C un 3 0.4939 g 46.52 s 29.791 °C 33.51 °C Use the following to determine the enthalpy of formation of magnesium oxide: Mg (s) + 2HCl (aq) MgCl₂ (aq) + H₂ (g) MgO (s) + 2HCl (aq) → MgCl₂ (aq)+ H₂O (1) H₂(g) + ½O₂ (g) → H₂O (l) -0.005191 °C/s -0.006452 °C/s -0.003932 °C/s -0.003809 °C/s MgO 0.5033 g 4 32.47 s 31.5714°C AH = (calculated in the experiment) AH = (calculated in the experiment) ΔΗ - 285.8 kJ/mol 35.27 °C AH = (determine using Hess's Law)
Transcribed Image Text:Room Temperature Reactant Trial Number Mass of reactant (from data) Moles of reactant (calculate) Initial time (ti) (from graph) Initial Temperature (Ti) (from the graph) Linear Curve fit slope (m) (from the graph) Linear Curve fit intercept (b) (from the graph) Final Temperature (T) (calculate from linear fit data) AT = T₁-Ti qwater calorimeter qrxu AHrxn 26.0°C Mg (s) + O2 (g) → MgO (s) Mg 1 0.2578 g 33.5 s 24.3°C Mg 37.23 °C 2 0.2551 g 41.05 s 29.055 °C MgO 41.72 °C un 3 0.4939 g 46.52 s 29.791 °C 33.51 °C Use the following to determine the enthalpy of formation of magnesium oxide: Mg (s) + 2HCl (aq) MgCl₂ (aq) + H₂ (g) MgO (s) + 2HCl (aq) → MgCl₂ (aq)+ H₂O (1) H₂(g) + ½O₂ (g) → H₂O (l) -0.005191 °C/s -0.006452 °C/s -0.003932 °C/s -0.003809 °C/s MgO 0.5033 g 4 32.47 s 31.5714°C AH = (calculated in the experiment) AH = (calculated in the experiment) ΔΗ - 285.8 kJ/mol 35.27 °C AH = (determine using Hess's Law)
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