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: When 1.00 L of 2.00 M Na2SO4 solution at 30.0°C is added to 2.00 L of 0.750 M Ba(NO3)2 solution at 30.0°C in a calorimeter, a white solid (BaSO4) forms. The temperature of the mixture increases to 42.

Problem

When 1.00 L of 2.00 M Na2SO4 solution at 30.0°C is added to 2.00 L of 0.750 M Ba(NO3)2 solution at 30.0°C in a calorimeter, a white solid (BaSO4) forms. The temperature of the mixture increases to 42.0°C. Assuming that the specific heat capacity of the solution is 6.37 J/°C ? g and that the density of the final solution is 2.00 g/mL, calculate the enthalpy change per mole of BaSO4 formed.