A gas is enclosed in a container at $35~\mathrm{m^3\,mol^{-1}}$ and has the following composition at $49\,\mathrm{^\circ C}$
$\ce{N_2} \ 2\,\% $
$\ce{CH_4} \ 79 \,\%$
$\ce{C_2H_6} \ 19 \,\%$
Assuming an ideal gas, calculate the partial pressure of each component (in kPa).
My working so far: I chose $100 \,\mathrm{mol}$ because I've been given percentages and it's a nice number to work with, and I multiplied this with $35 \,\mathrm{m^3\, mol^{-1}}$ to get $3500 \,\mathrm{m^3}$
I used $P=\frac{nRT}{V}$ to calculate an overall pressure but got $76\, \mathrm{Pa}$ which seems way too low. Have I done anything wrong?