Haber Process

[*sunsoldier*]

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Hey I need some help on question 8 from the 2008 CSSA question:

8. The Haber Process is an important industrial process used produce ammonia gas, NH; What volume of gas, measured at 100kPa and 25degrees, would produce 51.1g ammonia?

How exactly to i work this out?

Thanks

[kaz1]

Find amount of moles of ammonia, use stoichometry to find amount of moles of Hydrogen and Nitrogen. Multiply ideal gas volume with the amount of moles Nitrogen and Hydrogen.

[astroe]

Haber process:
N2(g) + 3H2(g) <-> 2NH3(g)

m/M = 51.1g/(14.01+3x1.008)
= 2.99988259 moles.

Since 2.99988259 moles is equivalent to 2 moles of 2NH3, and since there is 4 moles on the left side, you double it.

Hence, moles of reactants = 5.99976518 moles.
1 mole of ideal gas = 24.79L @ 25C, 100kPa.

So, 24.79L x 5.99976518 moles = 148.734179L !

I just copied the whole calculator readout but you should give it in as many sig. figs as the question states.


(Am I right? LOL
If I'm not I have serious problems considering Chem trials are tomorrow)

[mitchell.j.bell]

Originally Posted by astroe

Haber process:
N2(g) + 3H2(g) <-> 2NH3(g)

m/M = 51.1g/(14.01+3x1.008)
= 2.99988259 moles.

Since 2.99988259 moles is equivalent to 2 moles of 2NH3, and since there is 4 moles on the left side, you double it.

Hence, moles of reactants = 5.99976518 moles.
1 mole of ideal gas = 24.79L @ 25C, 100kPa.

So, 24.79L x 5.99976518 moles = 148.734179L !

I just copied the whole calculator readout but you should give it in as many sig. figs as the question states.


(Am I right? LOL
If I'm not I have serious problems considering Chem trials are tomorrow)

Spot on mr astroe.