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: Calcium oxide and water react in an exothermic reaction:CaO(s) + H2O(l) → Ca(OH)2(s)       Heat of reaction (Rxn) = -64.8 kJ/molHow much heat would be liberated when 7.15 g CaO(s) is dropped into a be

Solution: Calcium oxide and water react in an exothermic reaction:CaO(s) + H2O(l) → Ca(OH)2(s)       Heat of reaction (Rxn) = -64.8 kJ/molHow much heat would be liberated when 7.15 g CaO(s) is dropped into a be

Problem

Calcium oxide and water react in an exothermic reaction:

CaO(s) + H2O(l) → Ca(OH)2(s)       Heat of reaction (Rxn) = -64.8 kJ/mol

How much heat would be liberated when 7.15 g CaO(s) is dropped into a beaker containing 152 g H2O.

a. 1.97 x 103 kJ

b. 508 kJ

c. 8.26 kJ

d. 547 kJ

e. 555 kJ

Solution

Concept: Thermochemical Equation 

Thermochemical equations relate heat to stoichiometry. Notice that it takes 1 mole of CaO to release 64.8 kJ of energy. 

View the complete written solution...