: For the following reactions predict the equilibrium shift. 5 CO(g) + I2O5(s) ß
ID: 304617 • Letter: #
Question
: For the following reactions predict the equilibrium shift.
5 CO(g) + I2O5(s) ßà I2(g) + 5 CO2(g) ?Ho = -1175 kJ
Change
Direction
of Shift
(product; reactant; or no change)
Change
Direction
of Shift
(product; reactant; or no change)
decrease in volume
d.
addition of CO2(g)
raise temperature
e.
removal of I2(g)
addition of I2O5(s)
f.
Lower heat/temp
Ni(s) + 4 CO(g) ßà Ni(CO)4(g) ?Ho = - 161 kJ
Change
Direction
of Shift
(product; reactant; or no change)
Change
Direction
of Shift
(product; reactant; or no change)
add Ni(s)
e.
decrease in volume
raise temperature
f.
lower temperature
add CO(g)
g.
remove CO(g)
remove Ni(CO)4(g)
h.
Decrease pressure
: For the following reactions predict the equilibrium shift.
5 CO(g) + I2O5(s) ßà I2(g) + 5 CO2(g) ?Ho = -1175 kJ
Change
Direction
of Shift
(product; reactant; or no change)
Change
Direction
of Shift
(product; reactant; or no change)
decrease in volume
d.
addition of CO2(g)
raise temperature
e.
removal of I2(g)
addition of I2O5(s)
f.
Lower heat/temp
Ni(s) + 4 CO(g) ßà Ni(CO)4(g) ?Ho = - 161 kJ
Change
Direction
of Shift
(product; reactant; or no change)
Change
Direction
of Shift
(product; reactant; or no change)
add Ni(s)
e.
decrease in volume
raise temperature
f.
lower temperature
add CO(g)
g.
remove CO(g)
remove Ni(CO)4(g)
h.
Decrease pressure
Explanation / Answer
In the FIRST CASE:
Let us consider Le Chatelier's principle:
a. Decrease in volume --- It will shift the equillibrium towards the Products as the number of moles in
the product side is less.
b. raise temperature ---- Equillibrium will shift towards left i.e. towards reactants.
c. Addition of I2O5 ---- Equillibrium will remain unchanged.
d. Addition of CO2 gas ---- Equillibrium will shift to the left , that is equillibrium will shift towards the side of the reactants.
e. Removal of I2 gas ---- Equillibrium will shift towards products.
f. lower heat/ temp --- Equillibrium will shift towards right, that is, equillibrium will shift towards the products.
IN SECOND CASE
a. Add nickel ---- No change in equillirium.
b. raise temperature ---- equillibrium shifts towards left, that is, towards the reactants.
c. Add CO gas ---- equillibrium shifts towards products.
d. Remove NiCO4 --- equillibrium shifts towards reactants.
e. decrease in volume --- equillibrium shifts towards products as number of moles towards products is less.
f. lower temperature --- equillibrium shifts towards products
g, remove CO --- equillibrium shifts towards products
h Decreases pressure --- equillibrium shifts towards reactants.
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