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: In which reaction does Kp = Kc? a) NO(g) + O2(g) <--> N2O3(g) b) N2(g) + O2(g) <--> 2NO(g) c) CaCO3(s) <--> CaO(s) + CO2(g) d) N2(g) + H2O(g) <--> NO(g) + H2(g) e) None

Problem

In which reaction does Kp = Kc

a) NO(g) + O2(g) <--> N2O3(g) 

b) N2(g) + O2(g) <--> 2NO(g) 

c) CaCO3(s) <--> CaO(s) + CO2(g) 

d) N2(g) + H2O(g) <--> NO(g) + H2(g) 

e) None

Solution

We are asked to choose among the given reactions for which Kp = Kc.


The concentration equilibrium constant Kc is related to the pressure equilibrium constant Kp by the equation:


Kp=KcRTn

Where:

R = ideal gas constant (0.08206 L∙atm/mol∙K)

T = temperature in Kelvin

∆n = change in gaseous moles


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