Download the App!

Get 24/7 study help with the Numerade app for iOS and Android! Enter your email for an invite.

The combustion of what volume of ethane $\left(\mathrm{C}_{2} \mathrm{H}_{6}\right)$ measured at $23.0^{\circ} \mathrm{C}$ and $752 \mathrm{mmHg}$, would be required to heat $855 \mathrm{g}$ of water from $25.0^{\circ} \mathrm{C}$ to $98.0^{\circ} \mathrm{C} ?$

Get the answer to your homework problem.

Try Numerade free for 7 days

Like

Report

$4.10 \mathrm{L}$

Chemistry 101

Chapter 6

Thermochemistry

Carleton College

University of Kentucky

University of Toronto

Lectures

05:27

In chemistry, a chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Both reactants and products are involved in the chemical reactions.

06:42

In chemistry, energy is what is required to bring about a chemical reaction. The total energy of a system is the sum of the potential energy of its constituent particles and the kinetic energy of these particles. Chemical energy, also called bond energy, is the potential energy stored in the chemical bonds of a substance. Chemical energy is released when a bond is broken during chemical reactions.

05:29

The combustion of how many…

05:19

The combustion of what vol…

06:57

The heat of combustion of …

01:12

A gaseous fuel mixture con…

01:30

Ethane $\left(\mathrm{C}_{…

04:56

How many liters of $\mathr…

05:56

So for this question, were asked to calculate the volume of ethane required to heat some water to some specific degrees. So the first thing that we're going to calculate is how much energy or heat is required to change 855 grams of water from a temperature of 25 degrees Celsius to 98. And in order to do that, we're gonna take advantage of the following formula. That sheet is equal to mass times the specific heat capacity. Times change in temperature, so we already know some basic information. You know that the mass of the water it's 855 grams. We know the specific keep capacity of water is 4.184 and then we can also calculate the change in temperature. We know that it's final temperature of 98 degrees Celsius and that its initial temperature it's 25 degree Celsius. So when you plug all of that into your calculator, you can see that's 261. Killer jewels of heat is required to make water raise that temperature, so now we have to relate that to the combustion of methane. So the first step that we have to do is we have to write down the balanced chemical equation for the combustion of ethics. So the unbalanced chemical equation we know you'll involved ethane. It will involve the burning of Oxford gas and the limit water vapor was was carbon dioxide. And now we need to balance this equation. So in order to balance it, you first know that there's two moles of carbon on the left side. But there's only one mole of carbon on the right side. In order to correct that, we're going to add to here. No, the last thing that we have to do was reactive, or the next thing they have to do is to look at the hydrogen now. So for the hydrogen, we see that there's six moles of hydrogen. But there's only three moles of hydrogen here, and nowhere else in the equation is hatred present. So to correct that and put a three so now it's balanced six and six, and finally, we just fit in the auction. So when you calculate how much oxygen is on the right side, we shouldn't. There's three here and their six year, so in total we need to produce nine work. There's not six. There's four there. So in total, we need to produce seven moles of auction Adams. So we can do that by changing the coefficient to seven over to that will keep this equation balanced. Now, for our purposes, I'm not going to multiply everything by two. And the reason why I'm not gonna do that is because we're only using this equation to find how much he is released per mole of the reaction. And we don't necessarily need to multiply by two and do that while you should multiply by two if you're trying to find the chemical equation, But once again, that's not a purpose. So I won't do that will make it the calculation a little bit easier. So you want to find the heat of this reaction, the standard entropy. So we confined how much he is released per mole of ethane. So I'll have to do is find the heats informations of the products and subtract out the heat information of one mole of ethane. And we can ignore the auction because once again it's an element and the Standard and flippy or the heats information for elements are zero. So well we have to do then is we know that there's two moles of you too, and we know that the heat information first year two is negative. 393.5 Killer jewels promote. We add three moles of H 20 and we know that the the heat of formation for that is negative. 285 0.8 to a jewels for more. The last thing we have to use it distract out one mole of ethane and you know that the huge information for that it's negative 83 0.8 to kill jewels. So then, when you plug all of that into your calculator will get the heat of that reaction is negative. 1561 killer jewels promote. So that is how much heat is released when there is one mole, a thing that is combusted. But we know that's not what we're trying to do. This case, we only need 261 Killer jewel diffuse. We want to find how many moles of ethane are required in order to do that. So we take 261 kill jewels. And we know that from the equation that 150 or 1561 killed Jules, 1561 killed jewels of U two released for every one mole of the thing. And so then when you multiply this out, we know that approximately around the sixth of them all of a thing is required in combustion to produce 261 killer joules of heat. Now, the last thing that we have to do is now we've to find the volume of ethane and this and we have to relate that to the moles of the thing, which is what we're given. And in order to do that, you're going to use the ideal Gasol which says that PV equals and R t so we can rearrange that so that v equals and Artie overpay so we can plug the values that we know into this equation. We know that the amount of moles just from the previous part is your 0.167 miles. We know that our is a constant met zero point 08 to 1 leaders times atmosphere over moles times Kelvin multiplied by the change in temperature or the temperature. Not changed efforts, just the temperature of the gas. So we know that the temperature of the gas is a 23 degrees Celsius. But that's not useful for us because we didn't Kelvin. So to convert to Calvin you would simply add 200 and 73 that will give us Calvin. Then finally, we divide by the pressure. The pressure that you're given any problem is 7 52 Millet millimeters of Mercury or MME. Cheap. However, that's not a useful unit for us because, as you can see from the are constant, we want GM. So, in order, convert M. H G two atmospheres simply going to use this conversion that 1 80 m corresponds to 7 60 and she so when you multiply all of that together, you'll see that units will cancel out and will only be left with leaders when he plugged into calculator. You will see that the final answer is 4.10 leaders of anything, and that is the final answer

View More Answers From This Book

Find Another Textbook

Numerade Educator

03:16

Draw the Lewis structure of SO₃ (by following the octet rule on all atoms) a…

01:22

What is the pH of a 0.0355M KOH solution?

01:28

Write thermochemical equations for the formation of one mole of the followin…

01:59

What will happen to the following reversible reaction that is at equilibrium…

01:03

How many moles of Na+ ions are in 100.mL of 0.100M Na3PO4(aq) ?

Write oxidation and reduction half reactions for the following:S2- + NO3…

02:39

The mass of an alcohol used for an experiment in an organic chemistry la…

02:02

Calculate the pH of a buffer solution using the Henderson-Hasselbalch equati…

01:23

In the analysis of 0.7011 g of an impure chloride-containing sample, 0.9805 …

02:29

A solution of HClO4 was standardized by dissolving 0.3745 g of primary-stand…