Question

The following endothermic reaction is at equilibrium. 2 CO(g) + O2(g) 42 CO2 (g) What is the effect of the following changes on the position of the equilibrium? a) CO2 (g) is removed no shift b) The volume of the container is decreased by a factor of 2. shifts to make more product c) The temperature is decreased. shifts to make more products d) CO (g) is added no shift e) He (g) is added and the pressure doubles shifts to make more reactant

Answer 1

Given endothermic reaction is: 200 g) + 102 (8) 3 moles of gas 2002 (8) 2 moles of goo a C02(%) is removed : the om When CO₂ (g) is removed then concentration the product side ( Right) decreases. To undo this effect equilibrium shifts in the forward direction and produces more CO₂ (9) Ans a Shifts to make mose product 6 The volume of the Container is decreased: When volume is and the decreased then number of moles per unit volume increases pressure also increases. To undo this effect equilibrium shifts in the direction of lesser number of gaseous moles iie; in the forward direction and produces more CO2 (I) Ans (6) Shifts to make mose products Temperature is decreased For endothermic gtn: When temperatis is decreases them to undo this effect equilibrium swifts in the backward direction produces CO) and 02 and mode Ans Shifts to make more reactants

Cog) is added: when co(8) is added then concentration on the reactant Side increases. To undo this effect the equilibrium shifts in froward direction and produces mos CO2 Ans (d Shifts to make more products © He() is added and the pressure doubles : Не (3) is inert gas. a When inert gan is added to the equilibrium system at constant volume then the total pressure of the reaction will increase But the concentrations of the reactants and products will not change Hence there will be no effect on the equilibrium And е. No shift