NB Assume the densities of all solutions are 1.0 g/mL and their specific heat capacities 4.184 J/g .K RUN 1 Volume of tap water 50.0 mL 5.09 g Mass of KCI Initial Temperature of water, Ti 13.5 °C Final temperature of water, Tr 9.0 °C Change in temperature, AT RUN 2 Volume of tap water 50.0 mL Mass of KCI 5.17 g Initial Temperature of water, Ti 14.5°C Final temperature of water, Tr 9.5°C Change in temperature, AT Given: Molar mass of KCl: 74.55 g mol-1 RUN 1 Calculation of q, in J (qr = [Don't round] RUN 2 Calculation of q, in J (q, = – ąsoln) qsoln) [Don't round] Calculation of Enthalpy Change, AH in kJ mol-1 [Don't round] Calculation of Enthalpy Change, AH in kJ mol-1 [Don't round]
NB Assume the densities of all solutions are 1.0 g/mL and their specific heat capacities 4.184 J/g .K RUN 1 Volume of tap water 50.0 mL 5.09 g Mass of KCI Initial Temperature of water, Ti 13.5 °C Final temperature of water, Tr 9.0 °C Change in temperature, AT RUN 2 Volume of tap water 50.0 mL Mass of KCI 5.17 g Initial Temperature of water, Ti 14.5°C Final temperature of water, Tr 9.5°C Change in temperature, AT Given: Molar mass of KCl: 74.55 g mol-1 RUN 1 Calculation of q, in J (qr = [Don't round] RUN 2 Calculation of q, in J (q, = – ąsoln) qsoln) [Don't round] Calculation of Enthalpy Change, AH in kJ mol-1 [Don't round] Calculation of Enthalpy Change, AH in kJ mol-1 [Don't round]
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
![NB Assume the densities of all solutions are 1.0 g/mL and their specific heat capacities 4.184 J/g .K
RUN 1
Volume of tap water
50.0 mL
5.09 g
Mass of KCI
Initial Temperature of water, Ti
13.5 °C
Final temperature of water, Tr
9.0 °C
Change in temperature, AT
RUN 2
Volume of tap water
50.0 mL
Mass of KCI
5.17 g
Initial Temperature of water, Ti
14.5°C
Final temperature of water, Tr
9.5°C
Change in temperature, AT
Given: Molar mass of KCl: 74.55 g mol-1
RUN 1
Calculation of q, in J (qr =
[Don't round]
RUN 2
Calculation of q, in J (q, = – ąsoln)
qsoln)
[Don't round]
Calculation of Enthalpy Change, AH in kJ mol-1
[Don't round]
Calculation of Enthalpy Change, AH in kJ mol-1
[Don't round]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F55a833aa-184f-434b-af3c-76ba8618462a%2F0c6593e6-2b25-42fe-b6d4-92948dc71382%2Fvq6g8je_processed.png&w=3840&q=75)
Transcribed Image Text:NB Assume the densities of all solutions are 1.0 g/mL and their specific heat capacities 4.184 J/g .K
RUN 1
Volume of tap water
50.0 mL
5.09 g
Mass of KCI
Initial Temperature of water, Ti
13.5 °C
Final temperature of water, Tr
9.0 °C
Change in temperature, AT
RUN 2
Volume of tap water
50.0 mL
Mass of KCI
5.17 g
Initial Temperature of water, Ti
14.5°C
Final temperature of water, Tr
9.5°C
Change in temperature, AT
Given: Molar mass of KCl: 74.55 g mol-1
RUN 1
Calculation of q, in J (qr =
[Don't round]
RUN 2
Calculation of q, in J (q, = – ąsoln)
qsoln)
[Don't round]
Calculation of Enthalpy Change, AH in kJ mol-1
[Don't round]
Calculation of Enthalpy Change, AH in kJ mol-1
[Don't round]
![Assume the densities of all solutions are 1.000 g/mL and their specific heat capacities 4.184 J/g .K
PART I
Reaction equation:
Volume of 2.0 M HCI
25.0 mL
Number of moles of HCI
Temperature of HCI
14.0 °C
Volume of 2.0 M NH4OH
25.0 mL
Number of moles of NH4OH
Temperature of NH4OH
14.0 °C
Initial Temperature, Ti
14.0 °C
Final Temperature, Tr
24.0 °C
Change in temperature, AT
Calculation of q, in J (q, = - 4soln)
[Don't round]
What is the enthalpy change (AH) in kJ mol-1, when 1 mol of acid is neutralized?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F55a833aa-184f-434b-af3c-76ba8618462a%2F0c6593e6-2b25-42fe-b6d4-92948dc71382%2Fmt64jm_processed.png&w=3840&q=75)
Transcribed Image Text:Assume the densities of all solutions are 1.000 g/mL and their specific heat capacities 4.184 J/g .K
PART I
Reaction equation:
Volume of 2.0 M HCI
25.0 mL
Number of moles of HCI
Temperature of HCI
14.0 °C
Volume of 2.0 M NH4OH
25.0 mL
Number of moles of NH4OH
Temperature of NH4OH
14.0 °C
Initial Temperature, Ti
14.0 °C
Final Temperature, Tr
24.0 °C
Change in temperature, AT
Calculation of q, in J (q, = - 4soln)
[Don't round]
What is the enthalpy change (AH) in kJ mol-1, when 1 mol of acid is neutralized?
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 3 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.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