Question

What is the molar mass of (NH4)2O? Explain how you calculated this value.

Answer 1

@JFraser @ganeshie8

Answer 2

I think it is 52 g/mol is that correct?

Answer 3

http://www.wolframalpha.com/input/?i=%28NH4%292O+molar+mass

yes you are right

Answer 4

@wriddler. I think its actually 68g/mol if this is what you mean.
\[(NH _{4})_{2}O _{2}\]
The explanation is :
You take the first part (NH4)2. This says that there are
2 Nitrogens, at 14g/mol. = 28
(4H's) x 2. at H= 1g/mol, so 4*2*1=8.
Total that and get 28+8=36.

Next do the O2. This says there are 2 Oxygens. Each oxygen is 16g/mol
so, 2*16=32
Add that up 36+32 and get 68g/mol

Answer 5

but it said (NH4)2O, wouldnt that be like (NH4)2 + O essentially?

Answer 6

disregard what I last said I just realized something

Answer 7

the 2 in 2O is subtext

Answer 8

Do you mean \[(NH_{4})O _{2}\]

Answer 9

\[(NH _{4})_{2}O\]

Answer 10

thats what the question says

Answer 11

The answer that I saw somewhere else was:
N =14x2 = 28 H = 8 O = 16 Add them up 28 + 16 + 8 = 52, molar mass is written grams over moles or "g/mol"
so 52g/mol
but it doesnt seem very correct

Answer 12

@Australopithecus What do you think?

Answer 13

I'm pretty sure as you have stated, you have
2 (NH4)s. That means two of each element inside the bracket
Therefore
2 Nitrogens
4 hydrogens times 2
2N=28g/mol
8H= 8g/mol
Add those 2 and get 28+8=36

Next do the oxygen. 1 oxygen is 16g/mol

Add the 36+16 and you do get 52g/mol

Answer 14

okay thanks, mind helping me with one more?

Answer 15

\((NH_4)_2O\) certainly is a compound, it's ammonium oxide

Answer 16

yeah I'm just dumb :\

Answer 17

I should have known it exists durrrr