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: Consider the reactionNi (s) + 4 CO (g) → Ni(CO)4 (g).At 30°C and PCO = 1 atm, Ni reacts with CO (g) to form Ni(CO) 4 (g). At 200°C, Ni(CO)4 (g) decomposes to Ni (s) and CO (g). This means1. the forwar


Consider the reaction

Ni (s) + 4 CO (g) → Ni(CO)(g).

At 30°C and PCO = 1 atm, Ni reacts with CO (g) to form Ni(CO) (g). At 200°C, Ni(CO)(g) decomposes to Ni (s) and CO (g). This means

1. the forward reaction is endothermic.

2. adding an inert gas like argon favors the forward reaction.

3. the activation energy for the forward reaction is greater than for the reverse reaction.

4. a decrease in pressure favors the forward reaction.

5. K at 30°C is greater than K at 200°C.