Data: Csolution) 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: mMgo = 1.0 g T₁ = 28°C T₁ = 35 °C AT = Magnesium reaction data: mMg = 0.5 g T₁ = 28 °C T₁ = 46 °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 = q/n and fill in the blanks for each respective reaction. °C 5. Using the following series of reactions, calculate the heat of formation for magnesium oxide and the percentage error in the experiment. - MgO(s) + 2HCl(aq) MgCl₂(aq) + H₂O(l) Mg(s) + 2HCl(aq) MgCl₂(aq) + H₂(g) H₂(g) + 1/2O₂(g) - H₂O(l) The heat of formation reaction for magnesium oxide is kJ/mol AH₁ = AH₂ = kJ/mol AH3-285.8 kJ/mol Mg(s) + 1/2O2(g) → MgO(s) 6. Identify the experimental errors that would be a part of this experiment. Name
Data: Csolution) 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: mMgo = 1.0 g T₁ = 28°C T₁ = 35 °C AT = Magnesium reaction data: mMg = 0.5 g T₁ = 28 °C T₁ = 46 °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 = q/n and fill in the blanks for each respective reaction. °C 5. Using the following series of reactions, calculate the heat of formation for magnesium oxide and the percentage error in the experiment. - MgO(s) + 2HCl(aq) MgCl₂(aq) + H₂O(l) Mg(s) + 2HCl(aq) MgCl₂(aq) + H₂(g) H₂(g) + 1/2O₂(g) - H₂O(l) The heat of formation reaction for magnesium oxide is kJ/mol AH₁ = AH₂ = kJ/mol AH3-285.8 kJ/mol Mg(s) + 1/2O2(g) → MgO(s) 6. Identify the experimental errors that would be a part of this experiment. Name
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...
Related questions
Concept explainers
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Question
Please see screenshot and answer Questions 5 and 6 using the lab data given. Also, the enthalpy Magnesium oxide reaction is 1.18 kJ/mol and the enthalpy for the Magnesium reaction is 1.83 kJ/mol.
Thank you!
Transcribed Image Text: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:
mMgo = 1.0 g
T₁ = 28°C
T₁ = 35 °C
AT =
°C
Magnesium reaction data:
mmg = 0.5 g
T₁ = 28 °C
T₁ = 46 °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 = q/n 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.
AH₁ =
kJ/mol
ΔΗ2 =
kJ/mol
AH3 = -285.8 kJ/mol
MgO(s) + 2HCl(aq) → MgCl₂(aq) + H₂O(l)
Mg(s) + 2HCl(aq)
MgCl₂(aq) + H₂(g)
H₂(g) + 1/2O₂(g)
H₂O(l)
The heat of formation reaction for magnesium oxide is
Mg(s) + 1/2O2(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.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 4 steps with 7 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY