2. Iodine gas (I2) and chlorine gas (Cl2) react to form iodine monochloride (ICl) as shown according to the following re

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2. Iodine gas (I2) and chlorine gas (Cl2) react to form iodine
monochloride (ICl) as shown
according to the following reaction below at equilibrium. Consider
this reaction for the
questions below:
I2 (g) + Cl2 (g) ICl (g)

a. Draw the best Lewis Structure of the product that is produced
from this
reaction.
b. Identify the molecular geometry (shape) of the product that
is produced from
this reaction.
c. Identify the hybridization of the central atom(s) of the product
that is
produced from this reaction.
d. Identify the number of π bonds and σ bonds in the product that
is produced
from this reaction.
e. Is the product that is produced from this reaction polar or
non-polar?
f. Identify the type(s) of intermolecular forces that are present
in the product
that is produced from this reaction.
g. Write the equilibrium-constant expression (Kp) for the given
equilibrium
reaction, which is taking place in the production of iodine
monochloride.
h. Consider the equilibrium reaction given above. Consider an
experiment
where 0.250 mol I2 and 0.150 mol Cl2 are combined in a 1.00 L flask
at 727
C with a Kp value of 9.1. Calculate the concentrations of all the
reactant(s)
and product(s) at equilibrium.
i. If the Qp value for the reaction above, was found to be 595,
then what would
have to happen for the reaction to reach equilibrium (in which
direction
would the reaction have to shift)?
j. Predict the direction of shift if ICl is removed from the
equilibrium reaction
mixture.
k. Predict the direction of shift if Cl2 is removed from the
equilibrium reaction
mixture.
l. Predict the direction of shift if I2 is added from the
equilibrium reaction
mixture.
m. Predict the direction of shift if a catalyst is added to the
equilibrium reaction
mixture.