Ch.6 - Thermochemistry WorksheetSee 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
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 15.99 g sample of metal heated in a test tube submerged in 100.00°C water. It was then placed directly into a coffee cup calorimeter holding 51.95 g of water at 22.10°C. The temperature of the water increased to 24.99°C, determine the specific heat capacity of the metal. If the calorimete had absorbed 197.3 J and we factored that quantity into our calculation, what would the specific heat of the metal been?

Problem

A 15.99 g sample of metal heated in a test tube submerged in 100.00°C water. It was then placed directly into a coffee cup calorimeter holding 51.95 g of water at 22.10°C. The temperature of the water increased to 24.99°C, determine the specific heat capacity of the metal. 

If the calorimete had absorbed 197.3 J and we factored that quantity into our calculation, what would the specific heat of the metal been?