Homework #69

Moderators: Chem_Mod, Chem_Admin

Casey Collet 1I
Posts: 23
Joined: Fri Sep 26, 2014 2:02 pm

Homework #69

Postby Casey Collet 1I » Sat Nov 29, 2014 4:22 pm

In homework #69, I understand that the fact that the equilibrium constant is so small allows the reaction to strongly favor the reactants, but when doing similar problems how do we know that we are able to adjust the initial conditions according to the equilibrium constant?

K Honeychurch 1K
Posts: 27
Joined: Fri Sep 26, 2014 2:02 pm

Re: Homework #69

Postby K Honeychurch 1K » Sun Nov 30, 2014 10:23 pm

Adjusting the initial condition does not relate to the value of K being so small. In other words, we could adjust the initial condition for any value of K.
In this problem (and other problems with small K values), the very small K value allows us to ignore the change in the reactant (HCl) because 2x is much smaller than 4.0. With rounding, the final concentration of HCl will be 4.0 so we ignore the 2x to make solving the equation much easier.

Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 2 guests