In the following experiment, a coffee-cup calorimeter containing 100 mL of H2O is used. The initial temperature of the calorimeter is 23.0 °C. If 5.70 g of CaČl2 is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of solution AHsoln of CaCl2 is –82.8 kJ/mol. Assume that the specific heat of the solution formed in the calorimeter is the same as that for pure water: C, = 4.184 J/g.°C. Express your answer with the appropriate units. • View Available Hint(s) ? Value Units

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...
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Please answer question 9 part A

Calorimetry is a method used to measure changes
in enthalpy, or heat, that occur during chemical
processes. Two common calorimeters are constant-
pressure calorimeters and constant-volume (or
"bomb") calorimeters. Bomb calorimeters are used
to measure combustion and other gas-producing
reactions, in which the reaction is observed in a
strong, sealed vessel. A simple constant-pressure
calorimeter can be made from a foam coffee cup
and a thermometer, in which energy changes in a
reaction are observed via the change in
temperature of the solution in the cup. The idea
behind calorimeters is that if they are sufficiently
insulated from the outside environment, any energy
Part A
In the following experiment, a coffee-cup calorimeter containing 100 mL of H20 is used. The initial temperature of the
calorimeter is 23.0 °C. If 5.70 g of CaCl2 is added to the calorimeter, what will be the final temperature of the solution
in the calorimeter? The heat of solution AHsoln of CaCl2 is –82.8 kJ/mol.
Assume that the specific heat of the solution formed in the calorimeter is the same as that for pure water: Cs = 4.184
J/g.°C.
Express your answer with the appropriate units.
he chemical reaction will be
gained or lost
directly observable as a temperature and/or
pressure change in the calorimeter.
• View Available Hint(s)
HẢ
?
Value
Units
Transcribed Image Text:Calorimetry is a method used to measure changes in enthalpy, or heat, that occur during chemical processes. Two common calorimeters are constant- pressure calorimeters and constant-volume (or "bomb") calorimeters. Bomb calorimeters are used to measure combustion and other gas-producing reactions, in which the reaction is observed in a strong, sealed vessel. A simple constant-pressure calorimeter can be made from a foam coffee cup and a thermometer, in which energy changes in a reaction are observed via the change in temperature of the solution in the cup. The idea behind calorimeters is that if they are sufficiently insulated from the outside environment, any energy Part A In the following experiment, a coffee-cup calorimeter containing 100 mL of H20 is used. The initial temperature of the calorimeter is 23.0 °C. If 5.70 g of CaCl2 is added to the calorimeter, what will be the final temperature of the solution in the calorimeter? The heat of solution AHsoln of CaCl2 is –82.8 kJ/mol. Assume that the specific heat of the solution formed in the calorimeter is the same as that for pure water: Cs = 4.184 J/g.°C. Express your answer with the appropriate units. he chemical reaction will be gained or lost directly observable as a temperature and/or pressure change in the calorimeter. • View Available Hint(s) HẢ ? Value Units
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