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Ethyl alcohol is produced by the fermentation of glucose, CsH1zO6. CoHizOs(l) 2 CH:CHzOH() + 2 COz(g) AH = -82 kJ Find the heat of formation for CoH1zO6...

Question

Ethyl alcohol is produced by the fermentation of glucose, CsH1zO6. CoHizOs(l) 2 CH:CHzOH() + 2 COz(g) AH = -82 kJ Find the heat of formation for CoH1zO6

Ethyl alcohol is produced by the fermentation of glucose, CsH1zO6. CoHizOs(l) 2 CH:CHzOH() + 2 COz(g) AH = -82 kJ Find the heat of formation for CoH1zO6



Answers

The combustion of one mole of liquid ethanol, $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}$ , produces 1367 $\mathrm{kJ}$ of heat. Calculate how much heat is produced when 235.0 $\mathrm{g}$ of ethanol are combusted.

Then complice showing all I think. Inch 20 or cease, that's I won't. He wants to. So who? Los Push who? Oh, rebalance the reaction. Here it is. Cease. And here we should put six. So the number off ordered in other side six The flesh off this reaction, of course. Minus two. Close and 800 under eight. Up the other direction is the combustion off se. It's three. See ish tube orange. Okay, this is the combustion. Last port here is useless social plus hush people Insurrection six these years for also true on. Here it is too. And then you have cease. Okay, Have these two English and we don't know what is a little edge of this. It's under there for us. We have a summation off these two equations here. See special. The national goes six. So too It's six with The parts are sold to cause I'm here or two because what ever remains is this Okay? Six inch, but one Oh six. Yes. No, This it cost. He wants to Still who remains from here to I see or two last true. I see h three. No, I see. Plus to Oh, According to history rules, then Turkish. Because toe bigger in transformation equals British one under question. We have been two inch wound minus truthful signed 800 on eighth. We don't have the dentition number two, but it is to diminish with us. Here we have to one quick nice on dental ish off disconnect Red reaction Waas I dented bite from before waas minus living. Yeah, because who's minus 17? Tool from here in the image because it's minus 1300 60 paint, he usually.

So how do we calculate the Mueller heat capacity of ethanol? If we know its specific heat well, in order to do that, we need to know the units for more heat capacity which are jewels per mole degrees Celsius. And so if we know the value in calories per gram degree Celsius, we just have to do some dimensional analysis to figure that out. So if we have that value .586 calories program degree Celsius, we are going to convert calories into jewels. We know that there are 4.184 jewels in every calorie. And then we can use molar mass to convert grams into moles. And So we've got the more mass of ethanol is 46.08 g is one mole. And you can see that our grams cancel out our calories, cancel out. And we're left with the units of Mueller heat capacity. So when you wind up doing that math, you find out that the more heat capacity is 113 jules per mole degrees Celsius

All right, guys, we're doomed. Problem number ninety four of chapter five and chemistry. The central science. So the heat of combustion of ethanol is l would you see to h five. A wage is negative of one thousand three hundred sixty seven. Kill itches from all a batch of sauvignon blanc wine contains ten point six ethanol by mass. Assuming the density off the wine, too, is the wine is one point zero grams for leaders was the caloric content due to the alcohol in a six ounce glass of wine, which is one hundred seventy seven millimeters. So they wanted to find out that how many if we were to burn this wine, have how much of the energy would be due through the Ethel. So first we have to convert. Figure out how much ethanol we have, So we're going to take the density of the wine. We're going to multiply it by volume to get them, get the total amount of mass, and then we're going to multiplied by the fraction of ethanol to get just the amount of ethanol that just get the massive ethanol about the mass of the wine. Six. So this is going to equal eighteen went seven six grams of our ethanol. Now we're going to convert grams moles so our molecular weight of our ethanol we have to seize. That's going to be twenty four plus five. That's come between nine plus one. That's going to be thirty thirty, and then we're gonna have plus sixteen, which is forty six forty six grounds for mole. So we're going to divide eighteen point seven six six grams, divided by forty six grams per mole two eighteen point seven six. The vibe I forty six. But that's going to be equal to zero point zero point for one malls. And now we're going to and that we're going to multiply that time as times are as times are delta H value for the dotage of combustion and at ethanol. So we're gonna move by zero point for one more times. Negative one thirty six No. One three six seven killed Jules for more. So point point for one times thirty point for one MS thirteen sixty seven. That's going to be equal to five hundred and negative hundred and six sixty point four seven and kill a Jules. So now now they want to find the calorie content. So we're going to convert this jewels into food calories. So one Jule What? One killer Jule is going to be sorry. One food calorie. This is the food. Calorie is the kind of count the calorie content. You see, when you when you go, the story. You look at the food that that is the unit we use used to measure number of calories in a sample, so is equal to four point one eight. Kill it, Jules. So we're going to us and we can't drop the sign here is to be just one know about the magnitude of our of our sample four point four seven. Kill it, Jules. Times one Food calorie Hillary by four point one eight Killer Jules. They were going to put this into our calculator. Yes. So we're going to as so five. Sixty point four seven two by four points, one a. And that's going to be equal to one hundred thirty four point point zero eight food calories. And that is going to be the caloric content of our US of our ethanol in our sample in our wine

So let's start with our balanced equation. Okay, of the combustion of our ethanol. So we're gonna make to co two six H. Is so we'll make three H 20. And we'll balance that with a three in front of the oxygen delta H. For this is given as negative 13 67 killer jewels per mole of ethanol. So we've got 10% 10.6% ethanol. So let's start with R- 177 million lit of wine. And we've got a density. So let's change milliliters, two g of wine. So it's just one. So I have 177 g of wine And we know that 10.6% of it is ethanol. So we get 18.8 g of ethanol in our wine. Mm So let's go ahead and take those 18.8 g and let's change that to moles. Okay, so this is ethanol here. So one mole is 4608 g. And then each mall of methanol gives 13 67 Killer Jewels. So we know that will release negative 500 and 58 killer jewels.


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