Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Heat produced from HCl-NaOH reaction (J) assume the heat capacity of 1 M NaCl is 3.93 5681.94 5662.20 J/(g•*C) Molarity of HCI solution (M) 2.054 2.054 Moles of H20 formed in reaction (mol) Heat expected from moles of H20 formed (J) assume 57,320 J per mole of H20 Heat absorbed by calorimeter (J) (heat expected-heat actually produced) Heat capacity of the calorimeter (J/*C) (heat absorbed per degree of temperature change) Average heat capacity of the calorimeter (J/*C)

Heat produced from HCl-NaOH reaction (J) assume the heat capacity of 1 M NaCl is 3.93 5681.94 5662.20 J/(g•*C) Molarity of HCI solution (M) 2.054 2.054 Moles of H20 formed in reaction (mol) Heat expected from moles of H20 formed (J) assume 57,320 J per mole of H20 Heat absorbed by calorimeter (J) (heat expected-heat actually produced) Heat capacity of the calorimeter (J/*C) (heat absorbed per degree of temperature change) Average heat capacity of the calorimeter (J/*C)

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...
See similar textbooks
icon
Related questions
Question

Need help filling out the rest of this table 

 

Heat produced from HCI-NaOH reaction (J) assume the heat capacity of 1 M Nacl is 3.93 J/(9•°C) 5681.94 5662.20 Molarity of HCl solution (M) 2.054 2.054 Moles of H20 formed in reaction (mol) Heat expected from moles of H20 formed (J) assume 57,320 J per mole of H20 Heat absorbed by calorimeter (J) (heat expected-heat actually produced) Heat capacity of the calorimeter (J/°C) (heat absorbed per degree of temperature change) Average heat capacity of the calorimeter (J/°C)
Transcribed Image Text:Heat produced from HCI-NaOH reaction (J) assume the heat capacity of 1 M Nacl is 3.93 J/(9•°C) 5681.94 5662.20 Molarity of HCl solution (M) 2.054 2.054 Moles of H20 formed in reaction (mol) Heat expected from moles of H20 formed (J) assume 57,320 J per mole of H20 Heat absorbed by calorimeter (J) (heat expected-heat actually produced) Heat capacity of the calorimeter (J/°C) (heat absorbed per degree of temperature change) Average heat capacity of the calorimeter (J/°C)
Part A: Heat capacity calculations Run 1 Run 2 Initial temperature of HCl solution (°C) 20.2 20.9 Initial temperature of NaOH solution (°C) 21.1 20.4 Average initial temperature of HCI-NaOH solution (°C) 20.65 20.65 Maximum temperature of HCI-NAOH solution (°C) 34.2 34.1 Maximum temperature change for reaction (°C) 13.55 13.45 Volume of HCl solution (mL) 49.6 49.6 Volume of NaOH solution (mL) 53.0 53.4 Total Volume of HCI plus NaOH solutions (mL) 102.6 103.0 Mass of final NaCI solution (g) 106.70 107.12 assume 1 M NaCI has a density of 1.04 g/mL Heat produced from HCl-N2OH reaction (J) assume the heat capacity of 1 M Nacl is 3.93 J/(g•*C) 5681.94 5662.20
Transcribed Image Text:Part A: Heat capacity calculations Run 1 Run 2 Initial temperature of HCl solution (°C) 20.2 20.9 Initial temperature of NaOH solution (°C) 21.1 20.4 Average initial temperature of HCI-NaOH solution (°C) 20.65 20.65 Maximum temperature of HCI-NAOH solution (°C) 34.2 34.1 Maximum temperature change for reaction (°C) 13.55 13.45 Volume of HCl solution (mL) 49.6 49.6 Volume of NaOH solution (mL) 53.0 53.4 Total Volume of HCI plus NaOH solutions (mL) 102.6 103.0 Mass of final NaCI solution (g) 106.70 107.12 assume 1 M NaCI has a density of 1.04 g/mL Heat produced from HCl-N2OH reaction (J) assume the heat capacity of 1 M Nacl is 3.93 J/(g•*C) 5681.94 5662.20
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 7 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Crystal Structures
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
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS