Gas Laws Corrections: Calculating Volume & Molar Mass

[DB]

could u guys tell if I am right with these:
1)
a) calculate the volume occupied by 6.5 g of Nitrogen gas @ STP

\frac{1_{mol}}{28g_{N_2}}=\frac{x_{mol}}{6.5g}

x\sim0.23

\frac{101.3*V}{273*0.23}=8.31

so i got that 6.5 grams of N_2 is ~ 0.23 mol so using the ideal gas law i solved for V getting 5.15 L

b) calculate the volume occupied by this mass of gas at -40.0 C and 65.0 kPa

\frac{65*V}{233*0.23}=8.31

so i did the same thing as "a" except filled in those values of temperature(kelvin) and pressure, i got 6.9 L
2)
this one I am not so sure about:
what is the molar mass of a gas if 375 cm^3 have mass 0.800 g at 85 C and 100.7 kPa?
using the ideal gas law i did:

\frac{100.7*0.375}{358*n}=8.31

n\sim ~ 0.013 mol

then i divided 0.800g by 0.013 mol and got ~ 61.5 grams molar mass
is that right?
thanks in advance

 

[GCT]

you're using the wrong units, review your text or use common sense and use the correct units, remember standard temperature is 25C

 

[DB]

no you're thinking standard AMBIENT temp and pressure, these problems deal with STP, being 0C and 101.3 kPa

 

[GCT]

alright, check your answers with the that obtained by using the conversion factor 1mole/22.4L, part a) seems right, the third one seems fine by me