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What is the molecular formula of each compound if the empirical formula is CH and the actual molar mass of compound is 78 g/mole?

Answer 1

Naomi Aronson

The molecular formula is #C_6H_6#.

First, calculate the molar mass of the empirical formula, #CH# by adding the molar mass of carbon and hydrogen.

#12 + 1 = 13color(white)(l)g#/#molcolor(white)(l)CH#

Now, divide the molar mass of the molecular compound (actual molar mass) by the molar mass of #CH# to see how many times more massive the actual compound is.

#78/13=6# times more massive

After multiplying each atom in the empirical formula by 6, we know the molecular formula is #C_6H_6#.

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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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