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Given the following equation:2 C4H10 + 13O2 →→ 8 CO2 + 10H2OHow many moles of O2 are needed to produce2.51 mol of CO2?...

Question

Given the following equation:2 C4H10 + 13O2 →→ 8 CO2 + 10H2OHow many moles of O2 are needed to produce2.51 mol of CO2?

Given the following equation: 2 C4H10 + 13 O2 →→ 8 CO2 + 10 H2O How many moles of O2 are needed to produce 2.51 mol of CO2?



Answers

How many moles of propane gas, $\mathrm{C}_{3} \mathrm{H}_{8}$, react with $2.50 \mathrm{~mol}$ of oxygen gas? How many moles of carbon dioxide are produced? $$\mathrm{C}_{3} \mathrm{H}_{8}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2}\mathrm{O}(g)$$

First thing you have to do in this question is to consider the formula. So the equation the chemical formula ever seen here is C three H eight plus five oxygen, um, then reacts to farm three co two plus for each toe up. So this equation is balanced. We had to look, look around and figure out ways in which, um, for example, the hydrogen is re balance. There's eight hydrogen here, Rita multiply by four. But then the oxygen's are also not balance. We have multiplied by three and one side and five on the other as well as the carpenter. And so was everything is balanced. We can now move forward. Now that we know the different ratios really use the number off leaders of C three h h have to convert that the leaders of C E O. To so for every, um one c three h eight, we have to multiply it by three leaders of co two with one leader of C three h g at the bottom so that these cancel and CO. Two is now your unit. We got this three from up here in the question. So there's only one here in their three here, so we just do 2.33 times three, which gives you 6.99 Leaders of co two Great. It's now. It's only one more thing we have to change before you can plug into our equation. We have to change. Temperature were just given in Celsius to Kelvin. So we have to take the 24 Celsius and add 273 to convert into Calvin. So 24 plus 2 73 is 297. Finally, what we have to think about. What are we interested in this case? We want to know the moles we want to know. So we have to take PV equals energy. Divide both sides by r t to leave and by itself and we get an equals p V divided by party. Now we just have to plug in. You already given the, um, the pressure, which is 67 point you keep e eight we calculated leaders above, which is 6.99 leaders. We're gonna divide those two by the rate, which we just know is 8.314 which, um and the rate is multiplied by the temperature, which were the couple that had 297 covers. So we multiply these two together and these two together and divide that new waiter by the denominator. And after we do that simple math, we get a 0.19 Most Theo, too. Um, it's important to notice here that we have leaders here in the bottom which cancels leader in the top. Keep your canceled. Which is how we get, um, the moles. So we have 1.90 moles Theo, too.

In this question, we need to calculate the number of moles of each one of the reactant when the number of moles of water is provided. Now, before we can do that, by using the mole ratios, we know that we should check if the reaction equation is balanced or not. This one is not balanced. We have four carbons on the left hand side and one on the right hand side. So let's start off by trying to balance the number of carbon atoms, Putting a four year in front of the co. II, Then we have 10 hydrogen is on the left hand side and only two on the right hand side. Now, if I put it five in front of the water, this will cause an uneven number of oxygen atoms on the right hand side and on the left hand side we have di atomic oxygen, which means there will always be an even number of oxygen atoms on the left hand side. So therefore we need to work with an even number of oxygen atoms um for water And I'm gonna try 10. But if I do 10, This gives me 20 hydrogen on the um right hand side. So I have to put a two year in front of the butane gas. And this then affects the number of carbon atoms, which is then eight. So I have to have Um 8 CO2 on the right hand side. Now to check the number of oxygen atoms on the right hand side, We have 16 in CO2, and we have 10 in water. That's 26. So I can just put a 13 here in front of the oxygen gas and then the equation is balanced. Right now, I can use the number of more or the mole ratios in order to do the calculations. So the number of moles of butane gas C4 h 10 over the number of moles of the known substance, which is water um is going to be equal to Um story geometric coefficient of Putin gases too. So that's two over the short story geometric coefficient of water is 10. So now I have the number of moles of butane gas is equal to 2/10, which is 1/5 times the number of moles of water, which is Given us 2.5. Right, And that's simple um calculation that gives us a value of 0.50 moles. Next up, we need to calculate the number of moles of oxygen. Alright, oxygen gas over, once again as a denominator, I'm going to use the number of moles of water. And if I check my balanced equation, I see that I need to use a ratio of 13/10, 13, 13. So My number of moles of oxygen will be 13/10 Times the number of moles off water, which is given us 2.50. And then When I calculate this, I get a value of 3.25 moles for the oxygen. All right, so let's just check quickly. I had to balance my equation first before I could use more ratios in order to determine the unknown number of moles of both reacting to butane gas, and also for the oxygen.

So for this reaction were supposed to check that the number of moles of CO two produced if there is sufficient oxygen to react this entire reaction. So in general, we have this chemical equation, and we know that we're dealing with 3.6 old moles off CEO, and you want to find malls off CEO, too. So all we need to do is we need to look at the chemical equation and see the ratio between CEO and CO. Two. And considering that Oxygen has told us in, the problem is not limiting reactant, we don't need to worry about it. So look this chemical equation. We know that for every two moles of CEO produced, which is right here, two moles of CO two are produced, so the proportion is 2 to 2 was just simplifies to one. So in other words, we just get the exact same answer because our units cancel out and we get 3.6 miles with you. Two other words. For every mole of CEO that goes in a mole of CO two is produced 3.6. So is the final answer

Hi There in Probleble # 79. We are given moles of a reactant in a chemical reaction. And asked to calculate how many moles of one of the products will be produced. So we're going to need to use mole ratio to use mole ratio. We need a balanced equation which has been given to us As to C four H 10. I'm going to leave out the states of matter because they are not important for what we are doing in this problem. So that is combusting or burning in oxygen and it's producing carbon dioxide and water. So this is our balanced equation. And we are given moles of the Butane, the C four H 10. Specifically, We are given .41 moles and we are asked to determine how many moles of carbon dioxide will be produced. Okay, so this is what we're trying to determine. And from our balanced equation we can see the mole ratio for every two moles of the butane, we can produce eight moles of carbon dioxide. So it looks like we need to do a one step dimensional analysis using mole ratio. So what I mean by that is I'm going to start with what is given The point want 41 moles of C four age 10. And then from the equation we have inequality, two moles of C4 age 10 Will produce eight moles of CO two. So this 8/2 is the mole ratio. And this came from the coefficients in the balanced equation. And this is all I need to do for this problem because moles of beauty will cancel and my answer is going to be a moles of carbon dioxide. So, grabbing my calculator, calculating the answer and rounding it to two significant figures because .41 only has to We will get the answer of 1.6 Molds of CO two. Yeah. And that is our final answer. Mhm Yes.


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