Calculate the theoretical amount of co2 produced from 1000...

Calculate the theoretical amount of CO2 produced from 1.000 gallon of octane. Your final units should be lb CO2/gal fuel. The density of Octane is 0.750 g/mL; MW Octane = 114.2 g/mol; MW CO2 = 44.01 g/mol; 1.000 gal = 3.7854 L; 453.59 g = 1.000 lb. Then, calculate the theoretical amount of CO2 produced from 1.000 gallon of ethanol (lb CO2/gal). The density of ethanol is 0.789 g/mL, the molecular weight of ethanol is 46.07 g/mol, and the molecular weight of carbon dioxide is 44.01 g/mol. Why does ethanol emit less CO2 per gallon than gasoline?

Transcript

00:01 Okay, so for this question, this is going to be a whole lot of dimensional analysis.

00:06 And in dimensional analysis, we are going to take a value, and we are going to multiply it by a fraction, where the numerator and the denominator are equal to each other.

00:21 So in essence, what we're multiplying by is a fraction that is equal to one, but the units are different.

00:29 So let's say that the unit here is grams.

00:31 That would mean that i have to have some equivalent amount of grams in the denominator and whatever unit i want in the numerator.

00:41 So we will be able to cancel out like units that are in the numerator and the denominator.

00:48 And we will just consistently now on the next fraction, we will multiply by another fraction where the numerator and the denominator are equal.

00:55 But this unit will be in the bottom and a new unit will be on the top.

01:01 Seems complicated, but once you get the hang of it, it becomes second nature.

01:07 So the question itself gave a lot of different conversion factors.

01:14 And the conversion factor that had gallon in it said that it was 3 ,785 .4 milliliters for every one gallon.

01:29 That cancels out gallons.

01:31 Now, my next conversion factor has to have milliliters in it, and milliliters has to go in the bottom.

01:38 My density is 0 .150 grams for every milliliter.

01:45 So now that gets me into grams.

01:50 My molar mass is one mole for every 114 .2 grams.

01:58 That cancels out my grams.

02:00 Now, i am in moles of octane.

02:04 In order to switch from moles of one to moles of another, we need a mole ratio.

02:11 And i know that there are eight cs in octane.

02:16 So there will be eight co2s in the balanced equation for every 1, c8, h -18...

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