[lupok2001]

Good morning to everyone.

I need to calculate how many moles of carbon I have in 1ml of methane gas 95%.
This is how I have been thinking to proceed, I would like to ask your opinion:

Methane has a molar mass of 16,0435 and a density of 0,717 Kg/m^3

Being 1ml=1cm^3, I can rewrite the density as 0,717 x 10^(-3) g/ml

molarity of methane in 1ml is given by density/molar mass = 0,044 x 10^(-3)M = 0,044mM

being methane 95%, its adjusted molarity should be = 0,042mM

methane is CH4, so molarity of carbon should be the same as the one of methane.

Do you think it is right?

[Borek]

Good morning to everyone.

Hm, almost 5 p.m. here. Why do you sleep so long?

Methane has a molar mass of 16,0435 and a density of 0,717 Kg/m^3

You don't need neither molar mass nor density to solve this question. You should use ideal gas law.

molarity of methane

Molarity is a measure concentration. What you mean is not molarity, but number of moles.

Do you think it is right?

Not entirely, but numbers are OK.

[sjb]

Seems reasonably OK, but it would depend on what the other 5% is, and what percentage (w/w etc) you've reported.

If for instance the other 5% was butane, then your figures are in error, but if it were Xe, then there would be less issues.

[Borek]

Seems reasonably OK, but it would depend on what the other 5% is, and what percentage (w/w etc) you've reported.

Good points, missed that. But I suppose on HS level they can be safely ignored