Ch.14 - Chemical EquilibriumWorksheetSee 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: Use the following equilibria. SnO2 (s) + 2 CO (g) <==> Sn (s) + 2CO2(g)   Kc = 1.4 x1010 CO (g) + H2O (g) <==> CO2 (g) + H2 (g)   Kc = 9.0 x 1012 to calculate the Kc of this reaction Sn

Problem

Use the following equilibria.

SnO2 (s) + 2 CO (g) <==> Sn (s) + 2CO2(g)   Kc = 1.4 x1010
CO (g) + H2O (g) <==> CO2 (g) + H(g)   Kc = 9.0 x 1012

to calculate the Kc of this reaction

SnO2 (s) + 2 H(g) <==> Sn (s) + 2 H2O (g)  Kc= ?

A. 1.40 x 1010
B. 1.50 x 10-3
C. 1.13 x 1036
D. 1.73 x 10-16
E. 7.78 x 10-4