Chemistry molarity/molality problems

I'm very screwed, as I have a test on this stuff coming up and I can't even do these problems. Please, please, help.

Given: 1.00 g/mL as density of water.

1. What is the mass percent of HCl in an aqueous solution of 1.45M HCl? Assume the density of the solution is the same as the density of water.

For this question, I got 5.28%. Is that correct? Please show your work.

2. Using the same assumption as in the question above, determine the molality of HCl in an aqueous solution of 1.45M HCl.

For this question, I got 1.45 molality. Please show your own work whether my answer is correct or not.

I very much appreciate your help!

Question 1:
Molarity of HCl.

1.45 mol HCl
----------------
1L H2O

Assume 1L of water.

1 gram/1mL of water.

Due to assumption, mass of solution is 1kg.
Due to assumption, we have 1.45mol of HCl.

36.5 g HCl
-------------- Molar Mass of HCl.
1 mol HCl

1.45*36.5= 52.925 g HCl

59.925g HCl
----------------=5.9925%
1kg Solution

Question 2:
Molality is

Moles of Solute
-------------------
Kg of Solvent

From above, we know that the mass of solvent is equal to Mass(Solution)-Mass(HCl)=1kg -52.925g=940.075g H2O.

We know the moles of solute to be 1.45 mol.

Therefore, the molality is

1.45 mol
-------------------- = 1.5424 mol/kg.
.940075 kg H2O

Hope this helps!