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: McGraw-Hill Education
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Using Hess law answer the question from 1-4 . I will rate u
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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