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

Solution: An ice cube with a mass of 20 g at -20oC (typical freezer temperature) is dropped into a cup that holds 500 mL of hot water, initially at 86 oC.What is the final temperature in the cup? The density of

Problem

An ice cube with a mass of 20 g at -20oC (typical freezer temperature) is dropped into a cup that holds 500 mL of hot water, initially at 86 oC.

What is the final temperature in the cup? The density of liquid water is 1.00 g/ml the specific heat capacity of ice is 2.03 J/g-C the specific heat capacity of liquid water is 4.184 J/g-C the enthalpy of fusion of water is 6.01 kJ/mol.