[brandnewrocks13]

Ok.. so I'm having problems just with this last part of my problem.  Let me explain the problem and what I've done so far...
Here's my equation:
CH3NH2(aq)+H2O(l) --> CH3NH3+(aq)+OH-(aq)
the Kb of CH3NH2 is 4.4E-4 at 25 degrees C
I calculated the Delta Gstandard to be 19.1 kJ

So here's the question I'm having trouble with
What is the value of Delta G when [H+]=1.6E-8 mol, [CH3NH3+]=5.4E-4 mol, and
[CH2NH2]=.110 mol?

So I'm pretty sure that I'm going to need to use the equation Delta G=Delta Gstandard+RTlnQ.

I'm just not sure how to work the moles into the equation.  Do I need to set up the equilibrium expression Q?  I'm just not sure because I only have moles, no concentrations and no volume amounts.

Can some one help me out a little? Thanks
 

[Astrokel]

I'm just not sure because I only have moles, no concentrations and no volume amounts.

What is the value of Delta G when [H+]=1.6E-8 mol, [CH3NH3+]=5.4E-4 mol, and
[CH2NH2]=.110 mol?

why bracket when it is mol?

[brandnewrocks13]

i didn't really think about that, but it's listed in the problem as [H+]=1.6E-8 mol.
So that's kind of strange, maybe i should treat it as concentration?

[Astrokel]

i have no idea, check with your teacher or the answer?