Physics 198 Lecture Notes - Lecture 2: Reaction Quotient, Equilibrium Constant, Ideal Gas
Document Summary
A + b -> c + d rate = k[a][b] = how quickly [a] & [b] decrease and how quickly [c]&[d] increase rate depends on concentration of reacts which changes over time. A + b c + d forward rate(f) = k_f[a][b] A & b used at this rate and c & d produced at this rate. reverse rate (b) = k_b[c][d] C&d used at this rate and a&b produced at this rate k_b does not equal k_f until equilibrium is reached. Both the forward and reverse reactions are continuing but the concentrations will not change. No observable change at the bulk level [] become constant. Dynamic equilibria = forward and backward processes continue to occur, but no macroscopically observable change. Chemical equilibria can be approached from either direction. A + b c + d at equilibrium: rate(f) = rate(b) k_f[a][b] = k_b[c][d] at equilibrium. or k_f/k_b = k_c = [c][d]/([a][b] at equilibrium.
