Finding the Chemical Formula and Relative Molecular Mass

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Discussion Overview

The discussion revolves around a chemistry problem involving the determination of the chemical formula and relative molecular mass of a compound composed of elements Y and nitrogen (N). Participants explore the implications of given weight percentages and the relationships between the elements in the compound.

Discussion Character

  • Homework-related
  • Mathematical reasoning
  • Debate/contested

Main Points Raised

  • One participant expresses difficulty in approaching the problem and seeks help from others.
  • Some participants suggest that the chemical formula is implied in the problem statement, specifically noting the ratio of Y to N atoms.
  • Questions are raised about calculating the grams of nitrogen in a 100-gram sample and how this relates to the mass of element Y.
  • A participant proposes a solution involving calculations based on the percentages provided, arriving at a chemical formula of Y3N2 and identifying Y as magnesium (Mg).
  • Another participant challenges the assumption that the total mass must be 100 grams, indicating that while it simplifies calculations, it is not a necessary assumption.
  • There is a discussion about the validity of certain calculations, with one participant pointing out that proving 1=1 is not a valuable conclusion and that the choice of 100 grams is coincidental for this specific problem.

Areas of Agreement / Disagreement

Participants express differing views on the necessity of assuming a total mass of 100 grams for calculations. While some agree that it simplifies the problem, others argue that it is not a requirement. The discussion remains unresolved regarding the implications of this assumption and the correctness of the proposed solution.

Contextual Notes

Participants highlight limitations in reasoning, particularly regarding the assumption of total mass and its impact on the calculations. There is also a recognition that the specific mass of 100 grams may not apply universally to other compounds.

nineteen
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My chemistry teacher gave me this problem. I tried and tried, but I couldn't figure it out and the deadline is tomorrow. Please help me out here friends.

1. This is the problem :

In a compound which is made of element Y, weight percentage of Y is 72% and N( Nitrogen) is 28%. Also, 3 Y atoms are bonded with 2 Nitrogen atoms. Find the followings...
  1. Chemical formula of the compound.
  2. Relative molecular mass of Y.

Homework Equations

are :[/B]

n of molecular formula = Molar mass/ Formula mass of empirical formula

number of moles = mass/Molar mass

(at least I think these are the only equations used.)
​

The Attempt at a Solution

:
[/B]
The things is that, even though I tried I couldn't approach the question... I couldn't find a way to enter and continue doing. Therefore there is nothing like an attempt done to solve the problem. I am sorry if this contradicts with your procedure of this specific template.

Please help me out here.

 
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Isn't the chemical formula more or less given in the problem?

Knowing the mass of N and the its mass percentage in the compound should get you the molecular mass of the compound.
 
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If the compound contains 28% of nitrogen, how many grams of nitrogen in 100 grams of the compound? How many moles is that? What is the mass of the element Y present?
 
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DrClaude said:
Isn't the chemical formula more or less given in the problem?

Knowing the mass of N and the its mass percentage in the compound should get you the molecular mass of the compound.

Hey, thanks for helping out. Like you said, the chemical formula is the one said in the question itself right? It wasn't obvious to me at first, but now I tend to think so too.
 
Borek said:
If the compound contains 28% of nitrogen, how many grams of nitrogen in 100 grams of the compound? How many moles is that? What is the mass of the element Y present?

Thanks for helping out my friend. By the way, the chemical formula is N2Y3 right?
 
nineteen said:
By the way, the chemical formula is N2Y3 right?

Yes, that's what you were told.
 
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Borek said:
Yes, that's what you were told.
Thank you very much man!
 
Borek said:
If the compound contains 28% of nitrogen, how many grams of nitrogen in 100 grams of the compound? How many moles is that? What is the mass of the element Y present?

Hey I didn't understand what you said here. Except for the molecular formula thing, what you said here is a bit unclear to me. Can you please explain it further if you don't mind? Thank you very much in advance...
 
Here's my solution. If there is anything please correct me...

(Mass of N/Total mass) x 100% = 28
Therefore, total mass = 100g

(3 x Mass of Y/100g) x 100% = 72
Mass of Y = 24 g

Chemical formula = Y3N2
The element having a mass of 24 is Mg
Therefore; chemical formula is Mg3N2

R.M.M = (24x3) + (14x2)
= 100

​
 
  • #10
nineteen said:
Therefore, total mass = 100g

No, that's an incorrect conclusion. I told you to assume mass of the sample to be 100 g as it often simplifies understanding calculations when percentages are involved (but in general is never necessary).

But your final answer is OK.
 
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  • #11
Borek said:
No, that's an incorrect conclusion. I told you to assume mass of the sample to be 100 g as it often simplifies understanding calculations when percentages are involved (but in general is never necessary).

But your final answer is OK.

Thank you very much
 
  • #12
Borek said:
No, that's an incorrect conclusion. I told you to assume mass of the sample to be 100 g as it often simplifies understanding calculations when percentages are involved (but in general is never necessary).

But your final answer is OK.

By the way, why did you say we have to assume? I don't understand. In the question it says there are 2 Nitrogen atoms bonded with 3 Y atoms and so, I selected the mass of mass of nitrogen as 28, and thought that it is the amount of mass in the total sample that when taken as a percentage it gives us 28%. See just like this...

[(14x2)/Total Mass] x 100% = 28 14 is the mass of one Nitrogen
(28/Total Mass) x 100% = 28
(28x100)/28 = Total Mass
So, Total Mass = 100 in grams...

I mean like, why is thinking this way wrong? @Borek
​
 
  • #13
nineteen said:
(28/Total Mass) x 100% = 28
(28x100)/28 = Total Mass

You are just proving that 1=1, which is hardly an interesting and valuable conclusion. You can insert any value for 28 and it will still hold. It also happens this particular compound has a molar mass of 100 g/mol so it looks like 100 g is special here. It is completely accidental and it will not work for other compounds.
 
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  • #14
Borek said:
You are just proving that 1=1, which is hardly an interesting and valuable conclusion. You can insert any value for 28 and it will still hold. It also happens this particular compound has a molar mass of 100 g/mol so it looks like 100 g is special here. It is completely accidental and it will not work for other compounds.

Ok, got it. Thank you very much!
 

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