3. Mixing 1.00 mL of 1.00M HNO, and 1.00 mL of 1.00 M KOH causes the temperature of the two at 21.3°Č to become 31.2°C. Calculate the heat of neutralization. 4. In a coffee cup calorimeter, the temperature of 35.0 g of water drops from 20°C to 15.6°C when 9.0 g KBr is dissolved in it. Write a thermochemical equation for this.
3. Mixing 1.00 mL of 1.00M HNO, and 1.00 mL of 1.00 M KOH causes the temperature of the two at 21.3°Č to become 31.2°C. Calculate the heat of neutralization. 4. In a coffee cup calorimeter, the temperature of 35.0 g of water drops from 20°C to 15.6°C when 9.0 g KBr is dissolved in it. Write a thermochemical equation for this.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 113SCQ
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Instructions are in the image attached, kindly solve problems 3 and 4. Thank you!
Transcribed Image Text:Activity 3.9
Answer the following.
. Einanol weighing 3.56 g is burned in a constant-volume bomb calorimeter.
Consequently, the temperature rises from 15.17°C to 28.52°C. If heat
mol
kJ
capacity of the bomb plus water is 8.224 KJ find the heat of reaction in
2. A metal sample weighing 56.7 g at temperature of 98.0°C was placed in
50.0 g of water in a calorimeter at 26.5°C. At equilibrium, the temperature
of water and metal was 34.6°C. What is the specific heat of the metal?
3. Mixing 1.00 mL of 1.00 M HNO, and 1.00 mL of 1.00 M KOH causes the
temperature of the two at 21.3°C to become 31.2°C. Calculate the heat of
neutralization.
4. In a coffee cup calorimeter, the temperature of 35.0 g of water drops from
20°C to 15.6°C when 9.0 g KBr is dissolved in it. Write a thermochemical
equation for this.
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