8 8 pts Kp for the following reaction is 625 at 25 C 2 NOg

8. (8 pts) Kp for the following reaction is 6.25 at 25 °C. 2 NO(g) + Br2(g) 2 NOBr(g) The enthalpy change for the reaction at standard conditions is -16kJ. Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made: (a) Adding more Br2(g) (b) Decreasing the temperature (c) Removing some NOBr(g) (d) Increasing the container volume

Solution

According to Le Chatelier\'s principle if a change applied to a system in equilibrium the equilibrium will shift to counteract the effect of the change.

a)if we add more reactant then the reaction will shift towards right side.so if we add more Br₂ then the reaction will shift towards right side.

b)enthalpy change is negative here .so this is a exothermic reaction.for exothermic reaction if we decrease the temperature the equilibrium will shift to right side.

so if we decrease the temperature the equilibrium will shift to right side

c)if we remove some products the equilibrium will shift to right side.

so if we remove NOBr then the equilibrium will shift to right side

d)number of moles of reactant is greater than number of moles of product.So if we increase the container volume then the reaction will shift to left side.