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: Consider a 1.00 L solution of 0.150 M HCN (Ka = 4.9 * 10−10); Assume carbon is the central atom.  Indicate whether each statement is true or false.     A. There are more HCN molecules in the soluti

Problem

Consider a 1.00 L solution of 0.150 M HCN (Ka = 4.9 * 10−10); Assume carbon is the central atom. 

Indicate whether each statement is true or false.  

 

A. There are more HCN molecules in the solution than CN ions 

B. The acid reaction (corresponding to Ka) would have a ΔG° < 0 

C. Adding 0.150 moles of a strong base to this solution would make a buffer 

D. HCN is polar and has a linear shape 

E. The best Lewis structure would have a single bond and triple bond on C

F. HCN would exhibit hydrogen bonds with water