# The given percent composition of an organic compound is #48.76% "C"# and #8.04% "H"#. Its molecular mass is #"74 g/mol"#. What are its empirical and chemical formulas?

Since the empirical formula mass is the same as the molecular mass, the empirical and molecular formulas are the same,

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Find the Empirical Formula

The subscripts in an empirical formula indicate the lowest whole-number ratio of elements in a compound.

The molar mass of each element multiplied by the sum of its subscripts yields the formula mass for the empirical formula.

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To find the empirical formula:

- Convert the percentages to moles by assuming a 100 g sample.
- Find the simplest whole number ratio of the elements.
- Use this ratio to determine the empirical formula.

For carbon (C): (48.76% , C) → (48.76 , g) of C → (48.76 , g / 12.01 , g/mol) = (4.06 , mol , C)

For hydrogen (H): (8.04% , H) → (8.04 , g) of H → (8.04 , g / 1.01 , g/mol) = (7.96 , mol , H)

The simplest whole number ratio of C to H is approximately 1:2.

Therefore, the empirical formula is (CH_2).

To find the molecular formula:

- Calculate the molar mass of the empirical formula.
- Divide the given molecular mass by the molar mass of the empirical formula to find the ratio.
- Multiply the subscripts in the empirical formula by this ratio to get th

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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.

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