- Ch.1 - Matter, Measurement & Problem Solving106
- Ch.2 - Atoms & Elements97
- Ch.3 - Molecules, Compounds & Chemical Equations134
- Ch.4 - Chemical Quantities & Aqueous Reactions115
- Ch.5 - Gases98
- Ch.6 - Thermochemistry84
- Ch.7 - Quantum-Mechanical Model of the Atom49
- Ch.8 - Periodic Properties of the Elements81
- Ch.9 - Chemical Bonding I: The Lewis Model79
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory78
- Ch.11 - Liquids, Solids & Intermolecular Forces41
- Ch.12 - Solids and Modern Material35
- Ch.13 - Solutions66
- Ch.14 - Chemical Kinetics83
- Ch.15 - Chemical Equilibrium52
- Ch.16 - Acids and Bases107
- Ch.17 - Aqueous Ionic Equilibrium130
- Ch.18 - Free Energy and Thermodynamics74
- Ch.19 - Electrochemistry87
- Ch.20 - Radioactivity and Nuclear Chemistry50
- Ch.21 - Organic Chemistry143
Chapter 6, Problem 65
A silver block, initially at 58.5 °C, is submerged into 100.0 g of water at 24.8 °C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.2 °C. What is the mass of the silver block?
Video transcript
Titanium reacts with iodine to form titanium(III) iodide, emitting heat. 2 Ti(s) + 3 I2( g)¡2 TiI3(s) ΔH °rxn = -839 kJ Determine the mass of titanium that react if 1.55 * 103 kJ of heat is emitted by the reaction.
The propane fuel (C3H8) used in gas barbeques burns according to the thermochemical equation: C3H8( g) + 5 O2( g)¡3 CO2( g) + 4 H2O( g) ΔH °rxn = -2044 kJ If a pork roast must absorb 1.6 * 103 kJ to fully cook, and if only 10% of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast?
Charcoal is primarily carbon. Determine the mass of CO2 produced by burning enough carbon (in the form of charcoal) to produce 5.00 * 102 kJ of heat. C(s) + O2( g)¡CO2( g) ΔH °rxn = -393.5 kJ
A 32.5-g iron rod, initially at 22.7 °C, is submerged into an unknown mass of water at 63.2 °C, in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 59.5 °C. What is the mass of the water?
A 31.1-g wafer of pure gold, initially at 69.3 °C, is submerged into 64.2 g of water at 27.8 °C in an insulated container. What is the final temperature of both substances at thermal equilibrium?
A 2.85-g lead weight, initially at 10.3 °C, is submerged in 7.55 g of water at 52.3 °C in an insulated container. What is the final temperature of both substances at thermal equilibrium?