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Sat 14 Nov, 2009 06:51 pm
An initial mixture of nitrogen gas and hydrogen gas is reacted in a rigid container at a certain
temperature as follows:
3H2(g) + N2(g) ??" 2NH3(g)
At equilibrium, the concentrations are: [H2] = 5.0 M, [N2] = 8.0 M, and [NH3] = 4.0 M. What were
the initial concentrations of nitrogen gas and hydrogen gas that were initially reacted?
How do I go about doing this?? Im beyond confused. Thanks!
@magnifico,
In order to get two moles of NH3, you need three moles of H2 and one of N2. You have four moles of NH3, so how many moles of H2 and N2 were required to make that? Add that to what is still there and you will have the original concentrations of those two gases.
@engineer,
After I figure out how many moles are required to make 4 of NH3, how do I add that to what is still there??
@magnifico,
Even after the reaction reached equilibrium, you had 5M of H2 and 8M of N2 left. After you calculate the number of moles of H2 and N2 that reacted, you have to add 5 and 8 to the totals to see what you started with.
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