Scan_Doc0018 - Always determine which reactant is limiting...

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Unformatted text preview: Always determine which reactant is limiting. 3 .n The Concept of Limiting Reagent 111 Thus 8.93 X 10 2 mol N2 requires 2.68 X 10 3 mol H2 to react completely. However, in this case, only 2.48 X 10 3 mol H2 is present. This means that the hydrogen will be consumed before the nitrogen. Thus hydrogen is the limiting reactant in this particular situation, and we must use the amount of hydrogen to compute the quantity of ammonia formed: 2 mol NH3 2.48 X 10 3 mel-tf;: X = 1.65 X 10 3 mol NH3 3 mel-tf;: Converting moles to kilograms gives 1.65 X 10 3 ~ X 17.0 g NH3 = 2.80 X 10 4 g NH3 = 28.0 kg NH3 l~ Note that to determine the limiting reactant, we could have started instead with the given amount of hydrogen and calculated the moles of nitrogen required: 1 mol N2 2.48 X 10 3 mel-tf;: X = 8.27 X 10 2 mol N2 3 mel-tf;: Thus 2.48 X 10 3 mol H2 requires 8.27 X 10 2 mol N 2 . Since 8.93 X 10 2 mol N2 is actually present, the nitrogen is in excess. The hydrogen will run out first, and thus again we find...
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