Question

consider the equilibrium, I2(s)+5F2 (g) <---> 2IF5 for which of the equilibrium constant is 0.750 atm-3....

consider the equilibrium,

I2(s)+5F2 (g) <---> 2IF5

for which of the equilibrium constant is 0.750 atm-3. in a particular experiment, 10.0g of iodine and 1.05 atm of fluorine and 1.05 atm of iodinepentafluoride were introduced into an otherwise empty 5.00 L container at 25 degrees celsius. will the number of grams of iodine increase or decrease when equilibrium is established? justify your answer.

Please show work, thanks!

Homework Answers

Answer #1

Ans. Reaction quotient, Q = [IF5]2 / [F2]5

Note that being in solid state, the amount of I2 is NOT accounted.

            Or, Q = (1.05 atm)2 / (1.05 atm)5 = 0.864 atm-3

# Given – Equilibrium constant, Keq = 0.750 atm-3

# Since Q > Keq, the reaction will proceed to the LEFT/ Backward direction to establish the equilibrium.

Now, because the reaction proceeds in backward direction, there would be formation of more I2 from IF5. Thus, the number of grams of iodine will INCREASE.

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