Experiment 14Advance Study Assignment: Heat Effects and Calorimetry1. A metal sample weighing 147.90 g and at a temperature of 99.5°C was placed in 49.73 g of water in a calo-rimeter at 23.0°C. At equilibrium the temperature of the water and metal was 41.8°C.metala. What was At for the water? (At = tanal - tinitial)T左= 99.5%4t<(418を-23.6℃/8.8%18.8 °CH2049.739b. What was At for the metal?TE= 23,0°CAt = (48%-79.5)= 57.72-57.738こHow much heat flowed into the water? (Take the specific heat of the water to be 4.18 J/g°C.)°CC.AH=4,1E) = 1°C e latm99.5x 4.183907.983907.98)joules319.77d. Calculate the specific heat of the metal, using Equation 3.9ニmedt3407-48 J (14746) Cs (-57.7C)O4579joules/g°Ce. What is the approximate molar mass of the metal? (Use Eq. 4.)g/mol2. When 4.98 g of NaOH was dissolved in 49.72 g of water in a calorimeter at 23.7°C, the temperature of thesolution went up to 50.1°C.Is this dissolution reaction exothermic?Why?a.b. Calculate qH,0, using Equation 1.joulesc. Find AH for the reaction as it occurred in the calorimeter (Eq. 5).ΔΗ-joules(continued on following page)

g/mol 2. When 4.98 g of NaOH was dissolved in 49.72 g of water in a calorimeter at 23.7°C, the temperature of the solution went up to 50.1°C. Is this dissolution reaction exothermic? Why? a. b. Calculate qH,0, using Equation 1. joules c. Find AH for the reaction as it occurred in the calorimeter (Eq. 5). AH = joules

g/mol 2. When 4.98 g of NaOH was dissolved in 49.72 g of water in a calorimeter at 23.7°C, the temperature of the solution went up to 50.1°C. Is this dissolution reaction exothermic? Why? a. b. Calculate qH,0, using Equation 1. joules c. Find AH for the reaction as it occurred in the calorimeter (Eq. 5). AH = joules

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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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

Experiment 14
Advance Study Assignment: Heat Effects and Calorimetry
1. A metal sample weighing 147.90 g and at a temperature of 99.5°C was placed in 49.73 g of water in a calo-
rimeter at 23.0°C. At equilibrium the temperature of the water and metal was 41.8°C.
metal
a. What was At for the water? (At = tanal - tinitial)
T左= 99.5%
4t<(418を-23.6℃
/8.8%
18.8 °C
H20
49.739
b. What was At for the metal?
TE= 23,0°C
At = (48%-79.5)
= 57.72
-57.7
38こ
How much heat flowed into the water? (Take the specific heat of the water to be 4.18 J/g°C.)
°C
C.
AH=4,1E) = 1°C e latm
99.5
x 4.18
3907.98
3907.98)
joules
319.77
d. Calculate the specific heat of the metal, using Equation 3.
9ニmedt
3407-48 J (14746) Cs (-57.7C)
O4579
joules/g°C
e. What is the approximate molar mass of the metal? (Use Eq. 4.)
g/mol
2. When 4.98 g of NaOH was dissolved in 49.72 g of water in a calorimeter at 23.7°C, the temperature of the
solution went up to 50.1°C.
Is this dissolution reaction exothermic?
Why?
a.
b. Calculate qH,0, using Equation 1.
joules
c. Find AH for the reaction as it occurred in the calorimeter (Eq. 5).
ΔΗ-
joules
(continued on following page)

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