[gcatal]

Can someone give a sense of whether I'm doing this correctly?

The problem:

How many liters of NH3 can be produced at a temperature of 27 degrees Celsius and a pressure of 760 torr, if 20 moles of N2 are consumed?

Solution

N2 + 3H2 --> 2NH3

20 mol N2 X 2 mol NH3/1 mol N2

40 mol NH3


V of NH3=nRT/P
V=40 * .08206 * 300k/760 torr
V of NH3= 1.30 L

Is this correct? I think I'm getting tripped up around how to represent "if 20 moles of N2 are consumed". Thanks for any help.

[Borek]

40 moles of ammonia is OK - that's what you get from 20 moles of N₂. But you have used wrong value of the ideal gas constant, so your volume is wrong.

http://en.wikipedia.org/wiki/Ideal_gas_constant

Choose one that has correct units. 0.082 requires pressure in atm, you are given torr.