<p>How do I show the answer with the ICE Table? I only know how to get the answer without it.</p>
<p>13.43
An initial mixture of nitrogen gas and hydrogen gas is reacted in a rigid container at a certain temperature by the reaction</p>
<p>3H2 (g) + N2 (g) <-----> 2NH3 (g)</p>
<p>At equilibrium, the concentrations are [H2] = 5.0 M, [N2] = 8.0 M, and [NH3] = 4.0 M. What are the concentrations of nitrogen gas and hyrdogen gas that were reacted initially?</p>
<p>My explanation: There are 4 moles of NH3 or 2 moles of 2NH3. So we add 2 moles to the number of moles of N2 at equilibrium, which will be 8.0 + 2.0 = 10 M N2. For H2, you have to add a total of 6 moles because you add 2 for each H2, and there are three H2's. So my answer is [H2] = 11 M and [N2] = 10 M. This is the correct answer in the book, but how would you do it using the ICE table?</p>