4. You mix 50.0 mL. of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions and the calorimeter were initially at 21.4°C. The final temperature of the neutralization reaction was determined to be 41.2°C. The calorimeter constant was known to be 109.6 J/°C. DensityAqueous Solution = 1.00 g/mL Specific Heat of water 4.184 J/g.°C a. What is the total amount of heat evolved in this reaction? b. If 145 mmol of the monoprotic acid were neutralized in this reaction, what is the molar heat of neutralization (kJ/mole)?
4. You mix 50.0 mL. of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions and the calorimeter were initially at 21.4°C. The final temperature of the neutralization reaction was determined to be 41.2°C. The calorimeter constant was known to be 109.6 J/°C. DensityAqueous Solution = 1.00 g/mL Specific Heat of water 4.184 J/g.°C a. What is the total amount of heat evolved in this reaction? b. If 145 mmol of the monoprotic acid were neutralized in this reaction, what is the molar heat of neutralization (kJ/mole)?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter6: Thermochemistry
Section: Chapter Questions
Problem 127CWP: In a coffee-cup calorimeter, 150.0 mL of 0.50 M HCI is added to 50.0 mL of 1.00 M NaOH to make 200.0...
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Transcribed Image Text:4. You mix 50.0 mL. of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions and the calorimeter were initially at
21.4°C. The final temperature of the neutralization reaction was determined to be 41.2°C. The calorimeter constant was known to be 109.6 J/°C.
DensityAqueous Solution = 1.00 g/mL
Specific Heat of water 4.184 J/g.°C
a. What is the total amount of heat evolved in this reaction?
b. If 145 mmol of the monoprotic acid were neutralized in this reaction, what is the molar heat of neutralization (kJ/mole)?
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