Question

Describe the different ways to shift the equilibrium to the left for the following reaction:

2 A (s) + 2 BC (aq) arrow 2 AB (aq) + C2 (g). Justify your answer. ΔH = −352 kJ

Answer 1

@sweetburger @Kevin @jhonyy9

Answer 2

@Nnesha

Answer 3

@sshayer @AloneS

Answer 4

Sorry for waiting,
I had a job to do before..

Answer 5

2 A (s) + 2 BC (aq) arrow 2 AB (aq) + C2 (g). ΔH = −352 kJ
This is exothermic reaction, because ΔH < 0

The different ways to shift the equilibrium to the left for the following reaction:

1. "decrease reactant concentration, that's AB and C2 concentration"
OR
"increase product concentration, that's A and BC concentration"

2. exothermic : AB and C2
endothermic : A and BC
So to shift equilibrium to left we need to make the equilibrium to shift to endothermic by : "Increase the temperature"

3. 2 A (s) + 2 BC (aq) arrow 2 AB (aq) + C2 (g)
reactant coefficient : 2 + 2 = 4
product coefficient : 2 + 1 = 3
If we "decrease the pressure or increase the volume", then the equilibrium will shift to reaction with highest coefficient.

Answer 6

THanks Kevin!

Answer 7

You're welcome :D