Analysis of a compound shows that it contains 7.0 g nitrogen and 16.0 g oxygen. What is its empirical formula?

Answer 1

#NO_2#

The simplest whole number that describes the constituent atoms of a species is called the empirical formula.

By utilizing the specified masses along with the atomic masses of every component, we establish an empirical equation as follows:

#"Moles of nitrogen"# #=# #(7.0*g)/(7.0*g+16*g)xx1/(14.01*g*mol^-1)=0.0217*mol#.
#"Moles of oxygen"# #=# #(16.0*g)/(7.0*g+16*g)xx1/(15.999*g*mol^-1)=0.0435*mol#.

So, we have the molar quantities of nitrogen and oxygen, respectively. To get the empirical formula, we just divide by the molar quantity of nitrogen, which is the LOWEST of the two:

#N:(0.0217*mol)/(0.0217*mol)=1#
#O:(0.0435*mol)/(0.0217*mol)=2#
And thus the empirical formula is #NO_2#.

Keep in mind that we need to estimate the molecular mass in order to find the molecular formula.

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Answer 2

The empirical formula of the compound is N₂O₄.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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