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: Consider the following reaction: CH3OH (g) → CO (g) + 2 H 2 (g)       ΔH = +90.7 kJ(d) How many kilojoules of heat are released when 50.9 g of CO(g) reacts completely with H 2 (g) to form CH3OH(g) at

Solution: Consider the following reaction: CH3OH (g) → CO (g) + 2 H 2 (g)       ΔH = +90.7 kJ(d) How many kilojoules of heat are released when 50.9 g of CO(g) reacts completely with H 2 (g) to form CH3OH(g) at

Problem

Consider the following reaction: 
CH3OH (g) → CO (g) + 2 H 2 (g)       ΔH = +90.7 kJ

(d) How many kilojoules of heat are released when 50.9 g of CO(g) reacts completely with H 2 (g) to form CH3OH(g) at constant pressure?

Solution

We’re being asked to determine the heat (q) absorbed by the reaction of 50.9 g CO

The given reaction is:

CH­3OH (g)  CO(g) + 2 H2(g); ΔH = +90.7 kJ


From the balanced equation, we can see that the given ΔH˚rxn (+90.7 kJ) corresponds to 1 mole of CO


Recall that at constant pressure, heat is equivalent to enthalpy.



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