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1)Consider the following equilibrium at 972 K for the dissociation of molecular iodine into atoms of...

1)Consider the following equilibrium at 972 K for the dissociation of molecular iodine into atoms of iodine. I2(g) ----> 2 I(g); Kc = 1.40 ? 10?3 Suppose this reaction is initiated in a 3.4 L container with 0.067 mol I2 at 972 K. Calculate the concentrations of I2 and I at equilibrium.

* I got I2= 0.0135M and I= 0.0124 is this right?*

2)Consider the following equilibrium.
NH3(aq) + H2O(l) -----> NH4+(aq) + OH ?(aq)
What will happen to the equilibrium constant if the concentration of NH4+ increases through the addition of a small amount of NH4Cl(aq)

A) the equilibrium constant increases
B) the equilibrium constant decreases
C) the equilibrium constant remains the same

*I think its C ?*

*if you can only answer one question please answer #1*

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Answer #1

КС-Ί.yoxID ) 0-061 3. Ч C. 22L 3. Ч 0.0197-1

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