Question

5. For the following exothermic reaction, tell how the equilibrium will shift in response to... 2H2O2(aq) = 2H20(1) + O2(g) (a) allowing O2 to escape. (b) adding H20 [trick question!). (c) increasing the total pressure. (d) increasing the temperature. (e) justify your answer to part d.

Help please! Show work

Answer 1

a)

Removing product will shift the reaction in the direction of product as per Le chatelier Principle

So, Equilibrium moves to product side

b)

Adding solid or liquid doesn't affect equilibrium

So, No effect on equilibrium

c)

Increasing pressure will shift the reaction in a direction which have lesser gaseous molecules as per Le chatelier Principle

Here reactant has less gaseous molecule

So equilibrium will move to left

So, Equilibrium moves to reactant side

d)

Increasing Temperature will shift the reaction in a direction which absorbs heat as per Le chatelier Principle

Forward reaction is exothermic in nature

hence, backward reaction will be favoured

So, Equilibrium moves to reactant side

e)

Increasing Temperature will shift the reaction in a direction which absorbs heat as per Le chatelier Principle

Forward reaction is exothermic in nature

hence, backward reaction will be favoured