I hate Chemistry...

Bah, help me, I feel so thick x_x...

At a temperature of 107 degrees, the reaction:

CO(g) + 2H2 (g) (insert reversible arrow) CH3OH (g)

reaches equilibrium under a pressure of 1.59Mpa with 0.122 mol of carbon monoxide and 0.298 mol of hydrogen present at equilibrium with a vessel of volume 1.04dm3.

Assuming ideal gas behaviour determine the total number of moles of gas present. Hence calculate the number of moles of methanol in the equilibrium mixture.

Reply 1

charco

Study Forum Helper

PV=nRT
you have total P = 1.59Mpa
T=107+273= 380K
V=1.04

therefore n=PV/RT = (1590 x 1.04)/(8.314 x 380)
total moles of gas = 0.5234 moles

therefore moles of methanol = 0.5243 - (0.122 + 0.298) = 0.104 moles methanol present at equilibrium

Reply 2

J2K

Yeah, I just noticed that earlier today. Damn x_x... Need to top up on my Chem b4 the exam next year lolz... Been focusing on the Econ waaaaay too much.

Thanks =).

- Jeff

Reply 3

Ghetto_Princess12

Yes i hate chemistry too Worst subject i picked at A-level.

Reply 4

Anarchy Everywhere

The Charmed Ones

Yes i hate chemistry too Worst subject i picked at A-level.

Ditto.

Reply 5

OrangeRedYellow

Hi just looking at this question. Could someone please explain why the volume doesn't need to be in m^3 in the ideal gas equation ????

Reply 6

Pigster

Original post by Mathathonica

Hi just looking at this question. Could someone please explain why the volume doesn't need to be in m^3 in the ideal gas equation ????

You should win a medal, you've somehow managed to dredge up an eleven year old thread and expect and answer from anyone who is still here.

Fortunately, Charles still is.

Anyhoo, you should also have noticed that the pressure isn't the value given in the Q - there has been a bit of jiggery pokery on the values and units; perhaps you were expecting:

n=PV/RT = (1590000 x 0.00104)/(8.314 x 380)

But... that is the same thing.