Chemistry 1024A/B Lecture Notes - Lecture 6: Equilibrium Constant, Partial Pressure, Reaction Quotient

• School: Western University
• Department: Chemistry
• Course: Chemistry 1024A/B
• Professor: Zhifeng Ding

Document Summary

O far (cid:449)e"(cid:448)e assu(cid:373)ed that che(cid:373)ical reactio(cid:374)s ca(cid:374) o(cid:374)l(cid:455) (cid:373)o(cid:448)e i(cid:374) o(cid:374)e directio(cid:374). We represent the fact that reactions can proceeds in both directions by using the symbol: This represents the fact that a is in equilibrium with b. Because the reactions can proceed in both directions equilibrium will be established, where the concentrations [a] and [b] are in a fixed ratio. ---this ratio is known as the equilibrium constant; The value of k depends on the chemical nature of reactants and products, and on the temperature. [a] and [b] remain constant once they have reached their equilibrium values. The (cid:374)u(cid:373)(cid:271)er of (cid:373)ole(cid:272)ules goi(cid:374)g (cid:862)fro(cid:373) left to right(cid:863) i(cid:374) a give(cid:374) amount of time is equal to the (cid:374)u(cid:373)(cid:271)er of (cid:373)ole(cid:272)ules goi(cid:374)g (cid:862)fro(cid:373) right to left(cid:863) N2o4 is a colorless gas that is stable at low temperature. When it is heated (e. g. to 100 c), it forms no2.