The drawing below shows a mixture of...

The drawing below shows a mixture of molecules: key carbon hydrogen nitrogen sulfur oxygen chlorine Suppose the following chemical reaction can take place in this mixture: 2 H2(g) + O2(g) ? 2 H2O(g) Of which reactant are there the most initial moles? Enter its chemical formula: Of which reactant are there the least initial moles? Enter its chemical formula: Which reactant is the limiting reactant? Enter its chemical formula:

Transcript

00:03 There, in this question we are given this balanced chemical equation.

00:07 So any balanced chemical equation gives us the mole ratio.

00:12 What the mole ratio is, is the ratio in which the reactants react and the products are formed.

00:19 And that ratio comes to us from the coefficients in the balanced equation.

00:24 There's nothing in front of the oxygen, so it's understood to be a one.

00:27 So our mole ratio here is going to be two moles of hydrogen react with every one mole of oxygen, and they produce two moles of h2o.

00:40 Okay, well as we look here and we count up our molecules, we see that we have six molecules of the h2, we have four molecules of the o2.

01:04 Okay, and remember mole is just a multiple of molecules.

01:09 One mole is avogadro's number of molecules, 6 .02 times 10 to the 23rd.

01:17 So the number of molecules that we have here is directly proportional to the number of moles.

01:27 All right, so with that in mind, let's start answering these questions.

01:31 We want to know which reactant has the most initial moles.

01:40 Well, the most moles is going to be the h2, just by counting up there.

01:45 Most moles will be hydrogen.

01:48 The least moles, or the fewer moles.

01:51 I guess with only two things we can't talk about most and least, but we are anyway.

01:56 All right, so least moles would be the oxygen with only four molecules.

02:04 And then we want to know the limiting reactant.

02:07 Let's talk about what a limiting reactant is.

02:15 A limiting reactant is the reactant used up first in a reaction...

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