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: A 70.0 g piece of metal at 80.0°C is placed in 100 g of water at 22.0°C contained in a calorimeter like that shown in Figure 5.12. The metal and water come to the same temperature at 24.6°C. How much

Solution: A 70.0 g piece of metal at 80.0°C is placed in 100 g of water at 22.0°C contained in a calorimeter like that shown in Figure 5.12. The metal and water come to the same temperature at 24.6°C. How much

Problem

A 70.0 g piece of metal at 80.0°C is placed in 100 g of water at 22.0°C contained in a calorimeter like that shown in Figure 5.12. The metal and water come to the same temperature at 24.6°C. How much heat did the metal give up to the water? What is the specific heat of the metal?

Solution
  • Amount of heat can be calculated using the equation: 

Where q is the amount of heat in J; c as specific heat in J/goC; m is mass in grams; and ΔT as change in temperature in oC

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