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: In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water:CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔH = -890.0 kJCalculate the value of q (kJ) in th

Problem

In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water:

CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ΔH = -890.0 kJ

Calculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure.

a. -94.6 kJ

b. 32.7 kJ

c. 0.0306 kJ

d. -9.46 × 104 kJ

e. -0.0106 kJ