1) The Reaction has a K c = 1.0*10 -15 at 672 K. At equilibrium, a) Only product

Question

1) The Reaction

has a Kc = 1.0*10-15 at 672 K. At equilibrium,

a) Only products exist

b) only reactants exist

c) reactants predominate substantially

2) A 0.10 M solution of HI will ioninze to a greater extent than a 0.10 M solution of HF.

Why is that statement true?

Explain both answers please

1) The Reaction X+Y 2Z has a Kc = 1.0*10^-15 at 672 K. At equilibrium, a) Only products exist b) only reactants exist c) reactants predominate substantially 2) A 0.10 M solution of HI will ioninze to a greater extent than a 0.10 M solution of HF. Why is that statement true?

Explanation / Answer

1) X + Y <-----------> 2Z ; Kc = 1.0*10-15

Now, Kc = [Z]2/{[X]*[Y]} < 1

thus, at eqb., concentration of reactants are much higher than the products concemntration

Hence the correct option is:- (c)

2) The given statement is true because the H--I bond is much longer and thus much weaker than the H--F bond which is shorter and stronger.

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