# 7 04 chem flvs Limiting reagent Stoichiometry Video transcript We're told methanol, which is used as a fuel in racing cars and fuel cells, can be made by the reaction of carbon monoxide and hydrogen.

So this is the methanol right there. They're giving us grams of carbon monoxide. So carbon monoxide we have grams of it. And they're giving us 65 grams of hydrogen, of molecular hydrogen.

## Law of Partial Pressure

They're mixed and allowed to react. They say what mass of methanol can be produced? And then they say what mass of the excess reactant remains after the limiting reactant has been consumed? So that tells you this is a limiting reactant problem, that we have too much or too little of one of these two reactants.

These are the two reactants there. The one that we have less of is the limiting reactant and that'll dictate how much of the product 7 04 chem flvs can produce. And the one that we have more of is the excess reactant. But first we have to figure out which is the limiting and which is the excess. And before we even do that, we should always check that our equation is actually balanced. So let's just check that. On the left-hand side of this equation we have 1 carbon right there.

On the right-hand side we also have 1 carbon, so that looks good so far. On the left-hand side of the equation we have 1 oxygen, and on the right-hand side we have 1 oxygen. Looks good so far.

## The Mole Concept

Left-hand side we have 4 hydrogens, 2 times 2. On the right-hand side we have 4 hydrogens, 3 plus 1. So this is balanced so we can proceed to try to figure out what the limiting reactant is. So the way we want to do it is to figure out how many moles of each of these we're given, and then figure out how many moles the stoichiometric ratio that's required by this reaction.

We already know what it is. We know that for every two moles of hydrogen required, we require-- you can see it right here from the equation-- 1 mole of carbon monoxide. This is what the equation tells us, so let's see how many moles of hydrogen and how many moles of carbon monoxide we have.

The first place to start-- we've done this several times-- is what is the molecular weight of carbon monoxide? So carbon monoxide molecular weight-- let me write it here-- molecular weight for carbon monoxide. It's a carbon, has a molecular weight of it's good to memorize that, carbons and oxygens and hydrogens show up so frequently.

And then oxygen is So it's equal to a molecular weight of 28, which tells us that carbon monoxide, if we want to view it this way-- so let's do the carbon monoxide first. So we're dealing with the carbon monoxide. So we have grams of carbon monoxide, and we want to write this in terms of how many moles of carbon monoxide do we have.

## Equilibrium Lab by marissa brown on Prezi

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