CHM242H5 Lecture Notes - Exothermic Process, Endothermic Process, Equilibrium Constant
Document Summary
On non-deal gasses there are deviations that increase with lower temperature and lower density. For every chemical in the gaseous state there is some temperature in which it does behave ideally. Deviations from ideal behavior (p=a/v2)(v-b) = rt expand. Let v/v-b = v+b/v v2 = v2 b2. Tb= a/rt = 0. 2444/0. 02661 = 112k or -1010c. Unit 2: chemical equilibria (chapters 15-17: define in terms of rates and rates constants. Kb is the rate of backwards reaction to respect to time. Kf is the rate of forward reaction rf = bf [h2][i2] = kb [hi]2 = rateb. Equilibrium is when the rate of the backwards of forwards reactions are equal. K = kf/kb = [hi]2/[h2][i2] = 55. 3 at 700k. Le chatelier"s principle said that if anything is added or subtracted to a system then the system would try and change itself so it could be back to equilibrium. Exothermic and the reaction shifts to the left and k decreases.
