[Kdub]

I'm trying to complete an assignment and got kind of stumped on a couple questions. Here is the first question:

1. Complete combustion of 2.617g of a particular hydrocarbon yielded 8.846g CO2 and 1.811g of H2O. What is the empirical formula of this hydrocarbon?
Molar Masses
Hydrogen - 1.00794g/mol       Carbon - 12.011g/mol      Oxygen - 15.9994g/mol

This is what I did:
Moles CO2 = 8.846g / 44.0098g/mol
                = 0.201mol

Moles H2O = 1.811g / 18.0153g/mol
                = 0.100 mol

1:2 ratio H2O:CO2

So, empirical formula is C1H2

2. A 2.26g sample of a mixture of KCl and MgCl2 is treated with excess AgNO3 (aq). If 4.99g of AgCl are obtained, then what is the percentage by mass of KCl in the original mixture?
Molar Masses
KCl - 74.55g/mol    MgCl2 - 95.21g/mol      AgCl - 143.35g/mol


moles AgCl = 4.99g / 143.35 g/mol
                 = 0.034809 mol

that's where I got stuck and don't know where to go

Can some one help me out? Thanks

[AWK]

1. Water contains two hydrogen atoms - in molecular formula tou use atomic  ratio, not molecular one.
2.
 m1+m2=2.26 - mass of sample
m1/74.55+2xm2/95.21=0.034809 = moles of chlorine ions

[Kdub]

So then for 1. it would be C1H1?

and what would i do after finding moles of Cl...?

[Mitch]

and what would i do after finding moles of Cl...?  

find grams Cl.

[Kdub]

ok 1.23g Cl.
I just wanted some steps to follow not just a one step response, this assignment is due tonight guys i just want help on a question!