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: Suppose that the gas-phase reactions A → B and B→ A are both elementary processes with rate constants of 4.7 x 10-3 s-1 and 5.8 x 10-1 s-1, respectively.Which is greater at equilibrium, the partial pressure of A or the partial pressure of B?A(g) ⇌ B(g)

Solution: Suppose that the gas-phase reactions A → B and B→ A are both elementary processes with rate constants of 4.7 x 10-3 s-1 and 5.8 x 10-1 s-1, respectively.Which is greater at equilibrium, the partial pr

Problem

Suppose that the gas-phase reactions A → B and B→ A are both elementary processes with rate constants of 4.7 x 10-3 s-1 and 5.8 x 10-1 s-1, respectively.

Which is greater at equilibrium, the partial pressure of A or the partial pressure of B?

A(g) ⇌ B(g)

Solution

We are being asked to determine which will give a greater partial pressure at equilibrium for the given reaction

A(g)  B(g)

We are given the two elementary processes and their rate constant.


AB ; k = 4.7 x 10-3 s-1

 A ; k = 5.8 x 10-1 s-1


Recall: Associated with any reaction at equilibrium is the equilibrium constant K

Its numerical value determines if reactants or products are more greatly favored within a reaction


If K > 1      then the products > reactants and the forward direction is favored.

If K < 1      then the products < reactants and the reverse direction is favored.

If K = 1      then the products = reactants.


The equilibrium constant, K, can be expressed as the ratio of the forward and reverse rate constant

K = productsreactants=forward ratereverse rate

Solution BlurView Complete Written Solution