01:160:161 Study Guide - Final Guide: Joule, Endothermic Process, Bromine

• School: Rutgers University
• Department: Chemistry
• Course: 01:160:161
• Professor: Asbed Vassilia

Document Summary

Problems to prepare students for hourly exam ii: non acid-base equilibrium concepts, non acid-base equilibrium calculations, le chatelier"s principle, tavss 2/17. Non acid-base equilibrium concepts: 2no(g) + cl2(g) 2nocl(g) kp =1. 40 x 10. What is kp at 298 k for the reaction: nocl(g) no(g) + cl2(g) D. 5. 34 x 10-3: 2. 67 x 10-3. A. q must be equal to k at equilibrium. The larger the value of k, the farther the forward reaction proceeds toward completion. expression for q, because they do not change during the course of a chemical reaction. change for a system not initially in equilibrium. C. as the temperature increases, the value of k increases. D. the concentrations of pure solids and pure liquids are omitted from the. E. by comparing the value of q with k one can predict the direction of. Non acid-base equilibrium concepts: so2cl2(g) so2(g) + cl2(g) Flask x: 0. 50 mol so2cl2, 0. 10 mol so2, 0. 20 mol cl2 in 0. 50l.