A 0.0245 mg sample of nitrogen reacts with oxygen to form 0.0945 mg of the oxide. What is the empirical formula of this nitrogen oxide compound?
The empirical formula is
The reaction's equation is
We now need to find the ratios of these masses after converting them to moles.
I like to compile the calculations into a table from this point on.
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Calculate moles of nitrogen and oxygen. Determine the mole ratio. Empirical formula: N₂O.
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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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