What is the molecular formula of a compound that is 62.58% carbon, 9.63% hydrogen, 27.79% oxygen?

Answer 1

#C_6H_11O_2# is the simplest whole number ration that defines constituent atoms in a species, and is, therefore, the empirical formula.

As is the standard with these problems, we assume #100# #g# of compound, and break the percentages up into atoms.
In this mass, there are #(62.58*g)/(12.011*g*mol^-1)# #C# #=# #5.21# #mol# #C#.
And, #(9.63*g)/(1.00794*g*mol^-1)# #H# #=# #9.55# #mol# #H#.
And, #(27.79*g)/(15.999*g*mol^-1)# #O# #=# #1.740# #mol# #O#.
We divide thru, by the smallest molar quantity (#O#), and get (almost) the empirical formula: #C_3H_5.5O#.

We DOUBLE this formula because the empirical formula is the smallest WHOLE number ratio that characterizes constituent atoms in a species by definition.

#C_6H_11O_2#
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Answer 2

Given its composition, the compound has the molecular formula C₆H₁₀O₅.

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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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