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1. Calculate the temperature change for each reaction. 2. Calculate the energy released, in kJ, for each reaction using q = mcAT. 3. Calculate the number of moles, n, for magnesium oxide and magnesium. 4. Calculate the enthalpy of reaction, in kJ/mol using AH = qln and fill in the planks for each respective reaction. 5. Using the following series of reactions, calculate the heat of formation for magnesium oxide and the percentage error in the experiment.

1. Calculate the temperature change for each reaction. 2. Calculate the energy released, in kJ, for each reaction using q = mcAT. 3. Calculate the number of moles, n, for magnesium oxide and magnesium. 4. Calculate the enthalpy of reaction, in kJ/mol using AH = qln and fill in the planks for each respective reaction. 5. Using the following series of reactions, calculate the heat of formation for magnesium oxide and the percentage error in the experiment.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Magnesium Oxide Calorimeter Data: C(solution) = 4.18 kJ/kg/°C V(solutions) = 100 mL Density(solutions) = 1.0 g/mL C(solutions) = 1.0 mol/L Magnesium oxide reaction data: Magnesium reaction data: MMgo = 1.0 g T; = 28°C T; = 35 °C AT = mMg = 0.5 g Ti = 28 °C Tf = 46 °C °C AT = °C Calculations and Discussion 1. Calculate the temperature change for each reaction. 2. Calculate the energy released, in kJ, for each reaction using q = mcAT. 3. Calculate the number of moles, n, for magnesium oxide and magnesium. 4. Calculate the enthalpy of reaction, in kJ/mol using AH = gln and fill in the blanks for each respective reaction. 5. Using the following series of reactions, calculate the heat of formation for magnesium oxide and the percentage error in the experiment. MgO(s) + 2HCI(aq) → MgCl2(aq) + H2O(l) AH, = kJ/mol Mg(s) + 2HCI(aq) MgCl2(aq) + H2(g) ΔΗ- kJ/mol H2(g) + ½O2(g) H20(t) AH3 = -285.8 kJ/mol The heat of formation reaction for magnesium oxide is Mg(s) + ½02(g) → MgO(s) 6. Identify the experimental errors that would be a part of this experiment. Name at least two and state their effects on the calculations.
Transcribed Image Text:Magnesium Oxide Calorimeter Data: C(solution) = 4.18 kJ/kg/°C V(solutions) = 100 mL Density(solutions) = 1.0 g/mL C(solutions) = 1.0 mol/L Magnesium oxide reaction data: Magnesium reaction data: MMgo = 1.0 g T; = 28°C T; = 35 °C AT = mMg = 0.5 g Ti = 28 °C Tf = 46 °C °C AT = °C Calculations and Discussion 1. Calculate the temperature change for each reaction. 2. Calculate the energy released, in kJ, for each reaction using q = mcAT. 3. Calculate the number of moles, n, for magnesium oxide and magnesium. 4. Calculate the enthalpy of reaction, in kJ/mol using AH = gln and fill in the blanks for each respective reaction. 5. Using the following series of reactions, calculate the heat of formation for magnesium oxide and the percentage error in the experiment. MgO(s) + 2HCI(aq) → MgCl2(aq) + H2O(l) AH, = kJ/mol Mg(s) + 2HCI(aq) MgCl2(aq) + H2(g) ΔΗ- kJ/mol H2(g) + ½O2(g) H20(t) AH3 = -285.8 kJ/mol The heat of formation reaction for magnesium oxide is Mg(s) + ½02(g) → MgO(s) 6. Identify the experimental errors that would be a part of this experiment. Name at least two and state their effects on the calculations.
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