For the endothermic reaction H2(g) + I2(g) <---------> 2HI (g) which of 1) increasing the pressure 2) decreasing the volume 3) increasing the temperature will shift the equilibrium toward the products? Please show your reasoning! also how do I know how many moles are there for eachelements? For the endothermic reaction H2(g) + I2(g) <---------> 2HI (g) which of 1) increasing the pressure 2) decreasing the volume 3) increasing the temperature will shift the equilibrium toward the products? Please show your reasoning! also how do I know how many moles are there for eachelements?
Explanation / Answer
For endothermic reactions heat is taken from thesurroundings. H2(g) + I2(g) + Heat 2HI(g) a) Number of moles on the both sides is same. Pressure isrelated to the number of moles. As the pressure increasesshift takes place in such direction that will reduce theeffect. But here moles are common. So no effectof pressure. b ) Volume doesn't effect the above equilibrium.Because decreasing volume increases the pressure. But pressure hasno effect on above system. c) On increasing temperature equilibrium shifts in the endothermicside. All these are depending upon the Le Chatelier's principle.