Ch.6 - Thermochemistry See all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Calorimetry

See all sections
Sections
Internal Energy
Calorimetry
Hess's Law
Enthalpy of Formation
End of Chapter 6 Problems
Additional Practice
Units of Energy
Endothermic & Exothermic Reactions
Additional Guides
Enthalpy

Solution: A 19.78 g piece of nickel (specific heat of nickel = 0.444 J/g  oC) was heated to 103.5 oC and then plunged into a beaker containing 87.9 grams of water at 14.7  oC. Determine the final temperature of the metal after the system attains thermal equilibrium. (the specific heat of water is 4.184 J/g oC) A. 59.1 oC B. 44.4 oC C. 16.8 oC D. 12.5 oC E. 55.6 oC

Problem

A 19.78 g piece of nickel (specific heat of nickel = 0.444 J/g  oC) was heated to 103.5 oC and then plunged into a beaker containing 87.9 grams of water at 14.7  oC. Determine the final temperature of the metal after the system attains thermal equilibrium. (the specific heat of water is 4.184 J/g oC)

A. 59.1 oC

B. 44.4 oC

C. 16.8 oC

D. 12.5 oC

E. 55.6 oC