predict the effect of each of the follwing on the indicated equilibrium system in terms of....?

Question

....which reaction (forward, reverse, or neither) will be favored.

H2(g) + Cl2(g) <--> 2HCl(g) + 184kJ

a-addition of Cl2
b-removal of HCl
c-increased pressure
d-decreased temperature
e-removal of H2
f-decreased pressure
g-increased temperature
h-decreased system volume

Answer 1

Well I think you know that this is a le cheteier's principle (spelled wrong).

Look at the rxn.:

a.) adding Cl2 will make the equilibrium (label : Em) shift to the right. To make more products by reducing the reactant Cl2.

b.) Em right

c.) nothing because there is an equal amount of moles on both sides.

d.) right, to make more product. "Needs to warm up the system"

e.) left, to balance Em on both sides.

f.) nothing. same number of moles on both sides.

g.) left, "to cool down the system." Will make a negative H and hence compensate for the increased temp.

h.) nothing

Answer 2

Le Chateleier's Principle.

Whatever stress is created, the equilibrium is adjusted to relieve that stress.

Add more reactant, the forward reaction is pushed. Add more product, the reverse reaction is pushed

Add more heat, the endothermic direction is pushed, etc.

Pressure affects only if the moles are different on both sides. If so, then higher pressure pushes to fewer moles

Answer 3

a - to the right
b - to the right
c - no effect (equal moles of gas)
d - reaction is exothermic, so to the right
e - to the left
f - no effect, same reason as c
g - to the left (in the endothermic direction)
h - no effect, same reason as c