Question

Question 23 15 pts Consider the following reaction: N2O(g) + NO2(g) 3NO(g) AH = 155.7 kJ In which direction will the equilibrium be shifted by the following changes? 1. Adding N20 (Select] 2. Removing some N20 (Select] 3. Adding a catalyst (Select] 4. Adding NO [Select] 5. Increasing the temperature of the reaction mixture [ Select) 6. Decreasing the volume of the reaction vessel [Select] Question 24 10 pts A reaction vessel is charged with HI, which partially decomposes to molecular hydrogen and iodine.

Answer 1

me - Le-chatelice's I priciple various factes principle :- according to this after the director of react ooban • If equilibrium reactont Shift remore from the realban Left toward reactal Il product suy oware remere product from the realha equilibrium to increase produire concentrata I for ende thermmc reaction ( SH7o) It increases equlinina shy to rigut temperature vice-versa for exothermc reaction ( orke) I temperature increase equilerrim suy to left vice-versa Il pressure of realhon increases equilibrin sulfe whore number of gases moles is less (the effect of volume will be revesse of pressure P22) catalyse does not affect the equlibrin Scanned with CamScanner

Hanle for geven reaeben Ngo (g) + NO2(g) →300 g . SHE 155.719 . Reallon endotherme 6 Adding ngo al To increases concentrata of produe 3. YL Remoning some Na (left I to increase concennetu of Realtat sading a catayt No efters I 6 6 Adding No . [left] Increasing temperatur. I Rome Decreasing te volume Left endothom Because RY Scanned with CamScanner