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How much capsaicin (mg) is needed to prepare the capsaicin 005%_clear Medication following? Stick' #20 capsaicin tubes sodium stearate 7 g alcohol 65 g propyle...

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How much capsaicin (mg) is needed to prepare the capsaicin 005%_clear Medication following? Stick' #20 capsaicin tubes sodium stearate 7 g alcohol 65 g propylene glycol 25 g cyclomethicone 3 g

How much capsaicin (mg) is needed to prepare the capsaicin 005%_clear Medication following? Stick' #20 capsaicin tubes sodium stearate 7 g alcohol 65 g propylene glycol 25 g cyclomethicone 3 g



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Capsaicin, the compound that gives the hot taste to chili peppers, has the formula $\mathrm{C}_{18} \mathrm{H}_{27} \mathrm{NO}_{3}$ (a) Calculate its molar mass. (b) If you eat 55 mg of capsaicin, what amount (moles) have you consumed? (c) Calculate the mass percent of each element in the compound. (d) What mass of carbon (in milligrams) is there in $55 \mathrm{mg}$ of capsaicin?

Okay, so this is a fun little exercise which takes us through Simunic conversions and putting the concepts off moles and atomic mass. All of this putting this into context and we can actually put to good use here. So we're given a compound called capsaicin, which, interestingly enough, is, uh is found to give chili peppers Ah, hodge taste and were given It's molecular formula. So we're given what elements or how many atoms, uh, this compound is comprised of, So we see that has 18 carbon, 27 hydrogen, one nitrogen and three oxygen. And that is how the formula molecular formula is written out. So we're going to do a few things with this information. And first of all, we're asked to calculate the molar mass of cap season. So in order to do this, you actually need a periodic table handy, which I have Luckily, if you don't find one online or hey, just take my word for it. But I've looked up the atomic mass for each of the elements present in caps Assassin and you could find this number at the bottom of each square that Anel Ament occupies. There'll be a number rights below the letter, and this will be the atomic mass off that element. So carbon is 12, hydrogen is one, nitrogen is 14 and oxygen is 16. I rounded because it's very, very close to each of these integers. So in order to calculate the atomic mass off the whole compound, we need to incorporate or accommodate incorporate each element that is ah is existing right? So if carbon is 12 atomic mass, if that's his atomic mass, then we thio accommodate or, uh, take account for 18 carbons present, right? So it's not just 12, it's 12 times 18, which, if you did not know, is 216. Okay, 216 hydrogen is 27. The earth particular is easy enough. 27 times one is 27 hydrogen. We just have one. So that is 14 and the oxygen we have three. So three times 16. The math isn't very bad at all. It's 48. So add up all these things and what do we get? I will do it, sir. Verify? Leave it three or five. But let's always be certain before progressing on to further parts because I could definitely cause problems to arise later on. So we, um after computing that we know the atomic masses 305 and these are atomic mass units. So we're going to write this out is a M U. So the first part is simple enough. You just need a periodic table and need to do some multiplication and addition. So nothing too complicated. Conceptually. So now we have part B where we're told that we eat or potentially you eat 55 mg of cap season. So 55 mgs is consumed. General, if I'd be a spicy pepper or what The context is there but does not really matter. Um eso what amount off moles have we consumed? So this is a big exercise in unit two conversion and I will explain why in a second, so am you is atomic mass unit, but it is also known as grams per mole. So that is another way of understanding. What am you is referring thio that's more practical way, especially in this context. So we need to convert this 55 mg of capitation consumes two moles, and now we know we have the means to do so. So what? I mean, by this. So we know how many grams are per one mole, right? Because that's am you. So is 305 g per one mole. So we need to find out how many grams are consumed and then make sure that we have the right units. So first of all, there's a few different ways to do this. You could do it all in one fell swoop, or you could do it part by part. And I like doing it part by part just to be more organized in my head. So let's convert milligrams 2 g. If you don't know, 1 g is equivalent to 100 mg, right? You know, Millie, the prefixes referring to 100. So you just multiply this and then divide it or ice move the decimal place two points over. Because why make life hard when it could be easy? Right? 2.55 g is helmet. How many grams we consume? All right? Simple enough. So we have the amount of grams that we consume, and then we have the grams per mole. Two very important pieces of information. But how do we proceed? Mhm. Well, if you just multiply things across. We're not really changing anything. We need to think about canceling things out. And when we're looking at arithmetic when you cancel it, units, you want one unit to be on the top and when you need to be on the bottom when you're comparing. So beautiful thing is, you could just flip flop this because this is what this is grams per mole per one mole for am you grams per one mole So we can just write out as one mole, one mole of caps assassin. All this right cap season, right? C I. P has 305 g of atomic COMESA are atomic mass, right? Because atomic mass unit is grams per mole. So one mole of cap season has 305 grams. It's that easy. So now we have grams on top here, grams on bottom here. So they canceled and we have moles as the unit on top, which is perfect. So we just do 0.55 divided by 305 It's it's that simple. So let's look at the math. So 0.55 bye bye. 35 we are given 0.18 point 002 2.0 02 Moles. Okay. And that makes perfect sense. Because if you just think about it without the numbers in the way we know that for one mole it's 305 g, right? That's grams from all and were only consuming 0.55 g. That means we should have significantly less moles. Right? So that's how you can kind of just mentally check yourself. Think? Do these numbers make sense? Because sometimes things can be a little tricky When you're doing unit conversions. ESO is always gonna be able to conceptualize, right. So 305 grams per one mole. So for only having 10.55 grams, that significantly less than 305. So 3050.2 is significantly less than ah, one mole, Right, So that seems like it makes perfect sense. So now let's move on to part C. We're trucking along here, calculate the mass percentage of each element in the compound, so we're taking a step backwards. We're just looking at the compound, the molecular formula and the atomic mass units. Right. So, in order to do this, calculate the mass percentage of each elements. We know the total atomic mass, right? It's 305. We calculated it by adding everything up. So it's 305. So now we've got to take each component that we added up and divided by 305 because out of 305 how many atomic mass units ISAT responsible for? So let's do it for each element. So first off, you have carbon. We calculated to be 216 for, um 12 times 18. So that math, what's Destry? Ah, well, you know, we don't have to do this. We can just run this through, and they will give his decimal form. And if you want the percentage form just multiplied by 100 so there's no need to explain how to do this. I would just recommend using a calculator in our for the interest of time. So that's carbon. Next is hydrogen. I'll just write it out for you so that you have a good idea. So actually makes a little cleaner and then times 100 for percentage, you could do the same thing for the for the rest of them. You have 14 in the 48. Just do that divided by three or five times 100 I'll give you the percentage. Okay, So what Mass of carbon and milligrams is there in 55 mg of capitation. So now we're going back to the application part, which is beautiful. How the problem first gets you doing the conceptual part to understand how to, um gets the application part. So how maney, uh, milligrams of carbon is there in 55 mg of cap season. So this is really simple. We have to know the mass percentage of carbon which we showed you how to calculate it. So 216 divided by three or five. And you will get this calculation in front of you for the purpose of this problem. So 216 divided by three or five. It was 216 grams out of this, 305 that are carbon. This makes up 71%. Roughly so equals 71%. But in decimal formats, 0.71 right. Just C 0.71 is carbon. So of the 55 mg, how many of us is carbon? Well, you just multiply with the percentage by the total mass. Right, So times point 55 milligrams equals and let's do the math 0.71 times 0.55 The answer is point 39 which makes perfect sense. 390.39 You could do the same for each element. If you so desired, you just have to know the mass percentage, which I showed you how to calculate in part C. I guess label. This is Part E. It's part D. It's my my apologies there. So that is how you go about this problem. I think it's a very well thought out, um, exercise to demonstrate how to perform, you know, conversions and going from

This problem is from Chapter two, that is, atoms molecules in science and it is based on the most percentages off the substances. We have been given a compound that is cap season, which is a component off chili peppers and has the molecular formula C 18 age 27 en all three. In the first part, we have to find out the model mass of this compound. We have a topic masses off different elements in grams per mole. For carbon. It is 12 g for high erosion. It is 1 g for nitrogen. It is 14 graham in for oxygen. It is 16 graham. So more mass off this compound can be calculated by adding the atomic masses of different element present in its one molecule. So we have 12 to 18 gram for carbon plus 27 to 1 g for revolution. Yes, 14 grand for nitrogen, less 3 to 16 g for oxygen. And the mother mass can be calculated by adding these values and the motor mass comes out Toby three, not 5 g per mold. Next we have do find out the moles off this compound. If we consume 55 mg off this compound that is mass off the compound has given us 55 mg. We have to find out the number of moles off the compound. This will be calculated as and uh, the number of walls of the compound that is consumed on eating. 55 mg of this compound are 1.8 multiple bent and to the power minus fool. More. Next, we have to find out there mass percent off each element in the compound. This can be calculated as follows For carbon. The mass person will be 12. Motive Diamond 18, divided by 3. 95 in 200 this comes out to be 70.81% for hydrogen. It is 27 into one. They went by three. No. Five multiplied by 100. And this comes out Toby 8.85%. Then for nitrogen, it can be calculated as 14, divided by three. Note. Five multiplied by 100 this comes out to be 4.59%. And for oxygen, this comes out Toby. Three into 16. He went by three, not five multiplied the 100 and the value is 15.73% now in the last part, part B, we have toe find out the mass off carbon, which is present in 55 mg off baptism. Now, from this percentage, we know that 100 mg off compound has 70.81 mg off carbon. So 55 mg off compound we'll have touching 8.9 mg. That is mass off carbon will be 39 mg.

Hello, everyone. Today we do in Chapter 23 Problem 72 and this room masses to devices synthesis off. Why this molecule here starting from this starting material. And I'll draw that out on DH. Ah, it's firm from this and we can also use Miss Molecule here. It's moronic Esther on any other organic inorganic region. So let's see what we need to do. So let's count the carbons we want 234561234567 So it seems like we are actually gaining a carbon. So okay, and then we're also changing intensity of that. So let's see. So the carbon that we're going to be gaining is going to be from this Al Sakar mints, we have 123456 carbons with this Alfa Carbon being the 7th 1 So obviously we know that we need to change alcohol into some sort of Hey, light that once we dip, rotate this alfa position, we get a strong local folic and doing s into a backseat attack on this alcohol a life to gain this and then we do Hi draws his acid catalyst adrenal system spawn tasty carbolic solution to get a car books with acid in which we can change that into an alcohol chloride like this. So initial chloride like this? Sorry. So 1st 1 take this regent and I changes alcohol to Roman using PBR three. You see that we get this alcohol group, And then now if I take my storming through this Malin eights and I a strong base starting with offside, that's gonna give me a very strong car and island like this. And then if he's to react, I will get calculation at the alpha position. So you get 123456 like this. And if I had acid and heat, then you're going to get spontaneous hydrologists and decry box solutions. You'll just get Seo to plus your acid like this. Plus Theo, too, if I take this and I have Sokal to this, that I can change his too, from cover stomach acid to a nasal chloride. So you get seal. Oh, and this gives you your final product? Why

So here we're looking at the following reaction. So we have m.g. And to six h. 2. zero. This generates three G Ohh to add two and H three. So the molecular weight of MG three and 2, That is 100.9 grams per mole. And the weight of Manganese nitrate is 7.5 g. We can calculate the moles Where MG three and Two moles is equal to 7.50g, divide that by 109 grams per mole. That is equal to no point not 743, 3 moles. So, from the equation that we listed at the very top here, you can see that for two moles of ammonia, we generate one mole of MG three N two. So the ammonia produced. We need to double those moles. That is two times 9.97433. The molecular weight of N. O. Is about 17 g. So we can calculate the weight of ammonia produced Because we have two multiplied by 9.97433 for the moles Multiplied by 17 g per mole for the weight of Ammonia. The mass is therefore 2.53 g.


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