CHY 103 Chapter Notes - Chapter 143: Intermolecular Force, Reaction Quotient, North American Racing Team

104 views11 pages

Document Summary

If the reaction occurs in the gas phase, the more appropriate way to write the equilibrium would be write the equation as pressures: (cid:1837)(cid:3030)=[(cid:1829)](cid:3030)[(cid:1830)](cid:3031) [(cid:1827)](cid:3028)[(cid:1828)](cid:3029) (cid:884)(cid:1840)(cid:2870)(cid:1841)(cid:2873) (cid:886)(cid:1840)(cid:1841)(cid:2870)(cid:4666)(cid:1859)(cid:4667)+(cid:1841)(cid:2870)(cid:4666)(cid:1859)(cid:4667) (cid:1837)(cid:3017)=(cid:4666)(cid:1842)(cid:3015)(cid:3016)2(cid:4667)(cid:2872)(cid:1842)(cid:3016)2 (cid:4666)(cid:1842)(cid:3015)2(cid:3016)5(cid:4667)(cid:2870: the coefficients become the exponents in the expression. Can relate partial pressure of a to the ideal gas law: If we consider the following the equilibrium equation: We can relate to the first equation by substituting [a]: a relationship can be derived from this if the gases behave ideally. It is possible to represent the equilibrium constants in terms of pressures or concentrations and the two can be related to one another. Relating (cid:1837)(cid:3043) and (cid:1837)(cid:3030: the concentration of an ideal gas is the number of moles of a ((cid:1866)(cid:3002)) divided by its volume ((cid:1848)) in litres: We can rewrite the equilibrium constant (cid:1837)(cid:3030) as follows: (cid:1837)(cid:3030)=[(cid:1829)](cid:3030)[(cid:1830)](cid:3031) Substituting the equation of [(cid:1827)]=(cid:3017) into each concentration term in (cid:1837)(cid:3030):

Get access

Grade+
$40 USD/m
Billed monthly
Grade+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
10 Verified Answers
Class+
$30 USD/m
Billed monthly
Class+
Homework Help
Study Guides
Textbook Solutions
Class Notes
Textbook Notes
Booster Class
7 Verified Answers

Related Documents

Related Questions