Ch.6 - Thermochemistry WorksheetSee all chapters
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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 solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+ (ag) + Cl - (aq) → AgCI(s)       Δ H = - 65.5 kJ a) Calculate ΔH (kJ) for formation of 0.430 mol of

Solution: When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates: Ag+ (ag) + Cl - (aq) → AgCI(s)       Δ H = - 65.5 kJ a) Calculate ΔH (kJ) for formation of 0.430 mol of

Problem

When solutions containing silver ions and chloride ions are mixed, silver chloride precipitates:

 Ag+ (ag) + Cl - (aq) → AgCI(s)       Δ H = - 65.5 kJ 

a) Calculate ΔH (kJ) for formation of 0.430 mol of AgCl by this reaction.  

b) Calculate ΔH (kJ) for the formation of 6.00 g of AgCl.

c) Calculate ΔH (J) when 9.23 x 10-4 mol of AgCI dissolves in water.


Solution

First, we have to take note that we were given the standard enthalpy of formation for  AgCI(s)  and this is for 1 mole of  AgCI(s). 

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