# Volume of H2

## Homework Statement

Calculate the volume required to hydrogenate 50g of trans-carveol at STP.

PV=nRT
m=152g

## The Attempt at a Solution

I think I might have this one but just for clarification if I'm missing something. The amount of moles is 0.329 using the amount of carveol given and the molecular mass. So plugging in:

V=(0.329)(8.315)(298)/1
= 815L

Now, there are two double bonds in trans-carveol, so we need double the amount of hydrogen to hydrogenate the double bonds. So would it just be 815L x 2 = 1630L needed?

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Borek
Mentor
1 mole of gas at STP occupies 22.4 L, you have calculated there is 0.329 moles of carveol, that means you need LESS than 22.4 L, not many times more.

You are making an obvious error. Check your units.

Oh, silly me, it would be 0.08315, correct?

Ahh I see, thank you. So after I do the calculations to find the volume, was I right in saying originally that you double the volume since there are two double bonds?

Borek
Mentor
That would be my approach, it doesn't make it automatically right.