Write the equilibrium equation and Kf expression for the formation of:

Question

Write the equilibrium equation and Kf expression for the formation of: a. [AlF6]^-3 b. [Zn(CN)4]^-2 2. Suppose the following data are for the reaction: A==== Products. [A] Initial Rate 6 12 30 ? a.What rate should the ? be if the reaction is zero order? b.What rate should the ? be if the reaction is first order? c.What rate should the ? be if the reaction is second order?

Answer 1

 

Al³⁺ + F^- <=> [AlF]^3-  K1

[AlF]^3- + F^- <=> [AlF₂]^3-  K2

[AlF₂]^3- + F^- <=> [AlF₃]^3-  K3 ....

....etc.

Kf = [ [AlF₆]^3- ] / [A^l3+][F^-]⁶

 

Follow the same process for [Zn(CN)₄]^2-

 

For A <===> Products ... If I understand your presentation of data, 

You included the rates (6, 12, 30 and ?), but you didn't include the [A] at the corresponding rates.  For zero order, it won't matter, but for 1st and 2nd order one needs to know the [A].  Perhaps you meant that when [A] = 6, the rate = 30 and when [A] = 12, rate = ?.  But I'm not sure that's what you mean.

Rate = k[A]ⁿ where n is the order of the reaction.

For zero order, rate is independent of [A] and the rate will be the same at the different concentrations of A.

To find ? rate for 1st and 2nd order,

RATE = k[A^]n where n = 1 for 1st order and 2 for 2nd order.