Naked Science Forum
Non Life Sciences => Chemistry => Topic started by: Indranil on 26/08/2018 02:22:40
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Now my questions are below:
In the case of the first formula MO:
1. If the compound is 'MO' as a product, The reactant would be 'M +0.5 O2 = MO'
So if the total amount is 100 g (MO), M + 0.5 O2 =100g. From this equation in the left side, what will be the mass of O and M (not from the MO because I am able to calculate the mass of O and M from 'MO')?
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Now my questions are below:
In the case of the first formula MO:
1. If the compound is 'MO' as a product, The reactant would be 'M +0.5 O2 = MO'
So if the total amount is 100 g (MO), M + 0.5 O2 =100g. From this equation in the left side, what will be the mass of O and M (not from the MO because I am able to calculate the mass of O and M from 'MO')?
Your question is unclear. You are asking what the mass of O and M are and then right after you ask that you say "not from the MO". This sounds like a contradiction.
This also looks like a reposting of an earlier thread that you made: https://www.thenakedscientists.com/forum/index.php?topic=74427.0
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Now my questions are below:
In the case of the first formula MO:
1. If the compound is 'MO' as a product, The reactant would be 'M +0.5 O2 = MO'
So if the total amount is 100 g (MO), M + 0.5 O2 =100g. From this equation in the left side, what will be the mass of O and M (not from the MO because I am able to calculate the mass of O and M from 'MO')?
Your question is unclear. You are asking what the mass of O and M are and then right after you ask that you say "not from the MO". This sounds like a contradiction.
This also looks like a reposting of an earlier thread that you made: https://www.thenakedscientists.com/forum/index.php?topic=74427.0
You are right. I agree with you. The topic is the same but I wanted to ask different questions on this topic. I tried my best, still, the question is unclear. I am sorry for that.
Actually, I wanted to ask that 'MO' is a compound and in that compound if O is 27.6%. So the MO would be 100% or on the other hand, if I take 'MO' as 100g, so O would be 27.6g
As we know, If MO is 100g, So, M is (100-27.6) = 72.4g
So we get M = 72.4g and O = 27.6g
Now If I want to find the mole of O from the amount 27.6g, we get 1.725 moles of O from the amount 27.6g.
Now, If I want to find the mole of M from the amount 72.4g, how many moles of M from the amount of 72.4g we get? How to find it? here in this topic that's my question. Please explain.
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Now my questions are below:
In the case of the first formula MO:
1. If the compound is 'MO' as a product, The reactant would be 'M +0.5 O2 = MO'
So if the total amount is 100 g (MO), M + 0.5 O2 =100g. From this equation in the left side, what will be the mass of O and M (not from the MO because I am able to calculate the mass of O and M from 'MO')?
Your question is unclear. You are asking what the mass of O and M are and then right after you ask that you say "not from the MO". This sounds like a contradiction.
This also looks like a reposting of an earlier thread that you made: https://www.thenakedscientists.com/forum/index.php?topic=74427.0
You are right. I agree with you. The topic is the same but I wanted to ask different questions on this topic. I tried my best, still, the question is unclear. I am sorry for that.
Actually, I wanted to ask that 'MO' is a compound and in that compound if O is 27.6%. So the MO would be 100% or on the other hand, if I take 'MO' as 100g, so O would be 27.6g
As we know, If MO is 100g, So, M is (100-27.6) = 72.4g
So we get M = 72.4g and O = 27.6g
Now If I want to find the mole of O from the amount 27.6g, we get 1.725 moles of O from the amount 27.6g.
Now, If I want to find the mole of M from the amount 72.4g, how many moles of M from the amount of 72.4g we get? How to find it? here in this topic that's my question. Please explain.
Since the formula is MO, there are just as many moles of M as there are of O in any given amount of the substance.
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Now my questions are below:
In the case of the first formula MO:
1. If the compound is 'MO' as a product, The reactant would be 'M +0.5 O2 = MO'
So if the total amount is 100 g (MO), M + 0.5 O2 =100g. From this equation in the left side, what will be the mass of O and M (not from the MO because I am able to calculate the mass of O and M from 'MO')?
Your question is unclear. You are asking what the mass of O and M are and then right after you ask that you say "not from the MO". This sounds like a contradiction.
This also looks like a reposting of an earlier thread that you made: https://www.thenakedscientists.com/forum/index.php?topic=74427.0
You are right. I agree with you. The topic is the same but I wanted to ask different questions on this topic. I tried my best, still, the question is unclear. I am sorry for that.
Actually, I wanted to ask that 'MO' is a compound and in that compound if O is 27.6%. So the MO would be 100% or on the other hand, if I take 'MO' as 100g, so O would be 27.6g
As we know, If MO is 100g, So, M is (100-27.6) = 72.4g
So we get M = 72.4g and O = 27.6g
Now If I want to find the mole of O from the amount 27.6g, we get 1.725 moles of O from the amount 27.6g.
Now, If I want to find the mole of M from the amount 72.4g, how many moles of M from the amount of 72.4g we get? How to find it? here in this topic that's my question. Please explain.
Since the formula is MO, there are just as many moles of M as there are of O in any given amount of the substance.
Could you please explain the point above in a little more detail so that I can grasp the full concept?
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Could you please explain the point above in a little more detail so that I can grasp the full concept?
If the formula is MO, then there are just as many atoms of M in the substance as there are atoms of O. If you have a dozen oxygen atoms, then you must also have a dozen metal atoms. If you have a mole of oxygen atoms, then you must also have a mole of metal atoms.
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Could you please explain the point above in a little more detail so that I can grasp the full concept?
If the formula is MO, then there are just as many atoms of M in the substance as there are atoms of O. If you have a dozen oxygen atoms, then you must also have a dozen metal atoms. If you have a mole of oxygen atoms, then you must also have a mole of metal atoms.
Is it applicable for any compounds which match the formula MO such as 'MgO', 'CuO' etc?
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Could you please explain the point above in a little more detail so that I can grasp the full concept?
If the formula is MO, then there are just as many atoms of M in the substance as there are atoms of O. If you have a dozen oxygen atoms, then you must also have a dozen metal atoms. If you have a mole of oxygen atoms, then you must also have a mole of metal atoms.
Is it applicable for any compounds which match the formula MO such as 'MgO', 'CuO' etc?
Yes. That is the entire purpose of the formula: it states the ratios (of atoms) of the elements in a compound.
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Could you please explain the point above in a little more detail so that I can grasp the full concept?
If the formula is MO, then there are just as many atoms of M in the substance as there are atoms of O. If you have a dozen oxygen atoms, then you must also have a dozen metal atoms. If you have a mole of oxygen atoms, then you must also have a mole of metal atoms.
Is it applicable for any compounds which match the formula MO such as 'MgO', 'CuO' etc?
Yes. That is the entire purpose of the formula: it states the ratios (of atoms) of the elements in a compound.
you mean ration M:O = 1:1, Mg:O = 1:1, MnCl2= Mn :Cl2 = 1:2, Na₂S = Na₂:S = 2:1 etc? am I correct? Please let me know.
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you mean ration M:O = 1:1, Mg:O = 1:1, MnCl2= Mn :Cl2 = 1:2, Na₂S = Na₂:S = 2:1 etc? am I correct? Please let me know.
Yes, that is correct.
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MgO means one Mg nucleus for every O nucleus*
MnCl2 means one Mn nucleus for every two Cl nuclei
Na2S means two Na nuclei for every S nucleus
etc.
*(I say nucleus because it is most general--there are also electrons around, but we don't have to specify whether the nuclei are in atoms, ions, or molecules...)