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2 years ago

He molecular formula mass of this compound is 180 amu . what are the subscripts in the actual molecular formula?

Chemistry

1 answer:

mezya [45]2 years ago

5 0

I can't actually answer this one if the empirical formula is not given. Luckily, I've found a similar problem from another website. The problem is shown in the picture attached. It shows that the empirical formula is CH₂O. Let's calculate the molar mass of the empirical formula.

Molar mass of E.F = 12 + 2(1) + 16 = 30 g/mol

Then, let's divide this to the molar mass of the molecular formula.
Molar mass of M.F/Molar mass of E.F = 180/30 = 6

Therefore, let's multiply 6 to each subscript in the empirical formula to determine the actual molecular formula.
<em>Actual molecular formula = C₆H₁₂O₆</em>

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To determine the number of moles of carbon dioxide that is produced, we need to know the reaction of the process. For the reaction of HCl and sodium carbonate, the balanced chemical equation would be expressed as:

2HCl + Na2CO3 = 2NaCl + H2O + CO2

From the initial amount given of sodium carbonate and the relation of the substances from the balanced reaction, we calculate the moles of carbon dioxide as follows:

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Therefore, the amount in moles of carbon dioxide that is produced from 0.2 moles sodium carbonate would be 0.2 moles as well.

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2 years ago

Review the equation below. 2KClO3 mc012-1.jpg 2KCl + 3O2 How many moles of oxygen are produced when 2 mol of potassium chlorate

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Stoichiometry <span>of the reaction:

</span><span>2 KClO</span>₃<span>   =   2 KCl + 3 O</span>₂
  ↓ ↓

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hope this helps!

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3 years ago

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lukranit [14]

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Which organelle in the table is correctly matched with its function?<br> which one is it??

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$\huge\boxed{\sf Ribosomes}$

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$\rule[225]{225}{2}$

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1 year ago