An iron nail rusts when exposed to oxygen for the following...

An iron nail rusts when exposed to oxygen. For the following reaction, 0.142 moles of iron are mixed with 0.252 moles of oxygen gas. iron (s) + oxygen (g) ----> iron (III) oxide (s) What is the formula for the limiting reagent? _________________________ What is the maximum amount of iron(III) oxide that can be produced? __________________moles

Transcript

00:01 So to solve for this, let's write first to balance equation for this reaction.

00:05 So we have iron, that's fe, and then we have oxygen gas o2 to form f .e .2 -03.

00:12 So to balance this, going to write here two and then four here.

00:17 So that's the balance equation.

00:19 In order for us to identify the limiting reagent, we will calculate the mole ratio.

00:25 So mole ratio in this case will be the number of moles of the reactants divided by the coefficient of that reactant from the balance equation.

00:31 So for iron, we have 0 .142 moles divided by the coefficient of iron.

00:37 We have here four.

00:38 So divided by four, this will give us 0 .0355.

00:43 And then for oxygen gas, we have 0 .252 moles of oxygen gas divided by the coefficient of oxygen gas is, oh, i need to write here.

00:56 We have six oxygen on the right.

00:58 So we need to balance this also.

01:00 We need to adhere three.

01:01 Okay, so that's the balance equation, sorry.

01:04 And then the coefficient of oxygen gas is three.

01:07 So divided by three, this will give us 0 .084.

01:11 Whichever gives the smallest, small ratio will be the limiting reactant.

01:14 So that means iron is our limiting reactant.

01:18 So why did we have to identify the limiting reactant? because the amount of the limiting reactant will be the basis and the amount of the product that will be produced from the reaction...

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