1. Given the concentrations, calculate the equilibrium constant for this reactio
ID: 904919 • Letter: 1
Question
1. Given the concentrations, calculate the equilibrium constant for this reaction:
I2(g) +Cl2(g)2ICl(g)
At equilibrium, the molar concentrations for reactants and products are found to be [I2]=0.50 M, [Cl2]=0.60 M, and [ICl]=5.0 M. What is the equilibrium constant (Kc) for this reaction?
Express your answer using two significant figures.
2.The concentration of
I2(g) is increased to 1.5 M, disrupting equilibrium. Calculate the new ratio of products to reactants with this higher concentration of iodine. Assume that the reaction has not yet regained equilibrium.
Express your answer using two significant figures.
Explanation / Answer
1.
I2(g) +Cl2(g)2ICl(g)
Kc = [ICl]^2 / ( [I2] [Cl2] )
Kc = 5^2 / ( 0.5 * 0.6)
Kc = 83
2.
Q ( Reaction quotient)
Q = [ICl]^2 / [Cl2] [I2]
Q = 5^2 / ( 1.5 * 0.6)
Q = 28
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