compound containing Carbon, Hydrogen and Nitrogen only gave the following data on analysis: 0.1g of the compound on combustion gave 0.228g of CO2 and 0.124g of H2O. On further analysis, 0.1g of the compound gave NH3 which required 17.2 cm3 of 0.1M HCl for neutralization.
(i) How many moles of Carbon, Hydrogen and Nitrogen are there in 0.1g of the compound?
(ii) Deduce the empirical formula of the compound.
(iii) The relative molecular mass of the compound was found to be 116. What is its molecular
formular?
(iv) If the compound is known to be a primary amine, suggest one possible structure for the
compound.
Answers
Answer:
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Answer:
Yeah. Okay. So this scratching actually cast your basic on standing on the chemical formulas. So first let's organize the information the question provides a little bit. So it says a compound only contains uh, carbon hydrogen and the nitrogen. And now you have actually .1 g of the compound and combust ways auction. And the they used carbon dioxide which is .228g. And you have produced water which is .1 through four g. And you're also produced nitrogen. Uh, also some nitrogen compound, which you don't know. So the first question is to ask you, how many more is the carbon the hydrogen and nitrogen are in the compound? So we're going to actually find a direct relationship between the product and the reactant you refine for carbon, hydrogen and nitrogen. All of those elements in the product are totally coming from the reactions, which means the Morris of the carbon. The most of the hydrogen and the morse of nitrogen in the product are same in the um, the same actually in the reactivates. So we're now now here, the Morris of the carbon Simply equal to the more the carbon dioxide because it's 1-1 ratio right equals to the mass over the more mass, Which is .228 over 44. Yeah. Yeah. And the answer here is point oh, why one six more and saying more of the hydrogen here actually equals double moist of the Wall Street is one molecule has two hydrogen. See mass over more mass .125g over 18. Right? It's water and times too because you had to. And so it's actually equals two on the point oh one 38 more. And now we can calculate the most nitrogen. So here we can actually calculate the molar mass of the nitrogen first because we know the total mass is the .1 g minus massive the carbon in the compound minus miles of the hydrogen in the components. So the mass here is the .1g. The mass of the carbon equals two. The moors that was a carbon times more mass was a carbon minus the more massive the hydrogen times more of the hydrogen. It's just plug in the numbers. So the more mass of the carbon is .0518 times 12 miners .0138 times one. So now we can try to use a calculator. Do the calculations .1 -15 518 times 12 miners point 0138. And it's actually equals two around point 0244 grams. So the moors of the nitrogen just equal some mass of nitrogen over the more mass of nitrogen. So it's .024, all four g over 14, Which simple equals two point oh 17 one. Hey, more. So this is the answer for the first question. Then we go to the second question has reduced the empirical formula of the compound. So then we can just know the morse sure is the carbon over hydrogen And more nitrogen to simply equals two .0051 A ratio .0138. We should .001718. And you can just use your camp calculator to find the Uh huh. Yeah. Mhm. So here simply egos aids too long. So yeah, here, sweetie. So now we know it's safe. three H eight M 1. That's an empirical formula. And the third question around him, molecular mass of the compound is 116. So what is the molecular formula? So for this one, for the more mass of this empirical formula to simplify the formula, the more mass of this equals to 12 times three plus eight plus 14, which is equal through 58. and this 58 is actually half of the 116. Right? So the real formula should double the morse of the say this empirical formula. So it's actually say six, Age 16 and end to So this is an empirical formula and said if this compound is known to be a primary amine suggest they possible structure for the compound. Mm Mhm. Yeah. Yes. Yeah. So as you can say this is actually totally saturated. So from this formula because uh 16 hydrogen and there are two nitrogen six carbon, you know, it's a totally saturated. So in terms of formula it should be like uh no double bonds, you shouldn't have a double bonds. So and the primary amine means that the ammonia uh group, there's only one end of pneumonia in group that are linked to the carbon. So that's a primary I mean. So now we can look at that. So which means we can what we can do is first through the say six H. 16 framework, Right? So there are several choices. You have 1, 2, 3, 4, 5 6. We can have a chain, you can have a branch and those things. So I only ask us to suggest one. Right? So now like we can have much poorer than just give you all the choices here. So this carbon can be any location, right? And you don't have to have this. Then you can just put your ammonia group at any position to ammonia group at any position of those chains. And this is the answer. So for example, you can have this stage two, stage to stage two, Then n. h. two Here, 1 to stage two, Sage too, Stage two and NH two like this. And this is the answer
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