How Do You Calculate the Empirical Formula for Nitrogen and Oxygen Compositions?

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In summary, the given percentages for N and O are 36.8% and 63.25%, respectively, in the first sample, and 63.6% and 36.4% in the second sample. At a weight of 16 for O and 14 for N, the mass of each element cannot be determined without the total mass of the sample. As for the string problem, it is impossible to determine the exact amount of black and white string without knowing the total length of the string.
  • #1
donniemsb_12
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1. 36.8% of N and 63.25% of O
2.63.6% of N and 36.4% of O
at wts: N=14 and O=16



answer it thanks!
 
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  • #2
donniemsb_12 said:
1. 36.8% of N and 63.25% of O
2.63.6% of N and 36.4% of O
at wts: N=14 and O=16



answer it thanks!

Imagine, for instance 100g of sample 1. What mass is N, what mass is O? How many moles of each?
 
  • #3
i don't know . that's the given of our teacher :(
 
  • #4
If I had 100 metres of string, and 54% was black, 46% white, how much would be black and how much white?
 
  • #5
what ? :))
 
  • #6
Do you know what % means?
 
  • #7
donniemsb_12 said:
1. 36.8% of N and 63.25% of O
2.63.6% of N and 36.4% of O
at wts: N=14 and O=16



answer it thanks!

Welcome to the PF.

This is schoolwork, so I've moved it to the Homework Help forums, per the PF Rules. Also part of the rules is that you mush show us your work, before we can be of help. We do not do your schoolwork for you.

Please show us your work toward a solution...
 

FAQ: How Do You Calculate the Empirical Formula for Nitrogen and Oxygen Compositions?

What is an empirical formula?

An empirical formula is a chemical formula that shows the simplest ratio of elements present in a compound. It does not show the exact number of atoms, but rather the relative proportions of each element.

How is the empirical formula calculated?

The empirical formula is calculated by finding the molar mass of each element in a compound and then dividing it by the smallest molar mass. The resulting numbers are then multiplied by a common factor to get the simplest whole number ratio.

What is the difference between empirical and molecular formula?

The empirical formula shows the simplest ratio of elements in a compound, while the molecular formula shows the exact number of atoms of each element in a compound. The molecular formula is a multiple of the empirical formula.

Can the empirical formula be the same as the molecular formula?

Yes, if the compound has a simple molecular structure, the empirical formula and molecular formula can be the same. For example, the empirical and molecular formula of water is H2O.

Can the empirical formula be used to determine the molecular formula?

Yes, the empirical formula can be used along with the molar mass of a compound to determine the molecular formula. The molecular formula is a multiple of the empirical formula, so by knowing the molar mass, the molecular formula can be calculated.

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