Ch. 17 - Chemical ThermodynamicsWorksheetSee 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: For the reaction given below, ΔH° = -1516kJ and ΔS° = -432.8J/K at 25°C SiH4(g) + 2O2(g) →  SiO2(g) + 2H2O(l)  The reaction is spontaneous: a. only below a certain temperature b. only above a certai

Problem

For the reaction given below, ΔH° = -1516kJ and ΔS° = -432.8J/K at 25°C

SiH4(g) + 2O2(g) →  SiO2(g) + 2H2O(l) 

The reaction is spontaneous:
a. only below a certain temperature
b. only above a certain temperature
c. at all temperatures
d. at no temperatures
e. cannot tell from the information available.