Dalton’s atomic theory

[logistic_guy]

A \(\displaystyle 1.0\)-g sample of carbon dioxide \(\displaystyle (\text{CO}_{2})\) is fully decomposed into its elements, yielding \(\displaystyle 0.273\) g of carbon and \(\displaystyle 0.727\) g of oxygen. \(\displaystyle \bold{(a)}\) What is the ratio of the mass of \(\displaystyle \text{O}\) to \(\displaystyle \text{C}\)? \(\displaystyle \bold{(b)}\) If a sample of a different compound decomposes into \(\displaystyle 0.429\) g of carbon and \(\displaystyle 0.571\) g of oxygen, what is its ratio of the mass of \(\displaystyle \text{O}\) to \(\displaystyle \text{C}\)? \(\displaystyle \bold{(c)}\) According to Dalton’s atomic theory, what is the empirical formula of the second compound?

 

[The Highlander]

A \(\displaystyle 1.0\)-g sample of carbon dioxide \(\displaystyle (\text{CO}_{2})\) is fully decomposed into its elements, yielding \(\displaystyle 0.273\) g of carbon and \(\displaystyle 0.727\) g of oxygen. \(\displaystyle \bold{(a)}\) What is the ratio of the mass of \(\displaystyle \text{O}\) to \(\displaystyle \text{C}\)? \(\displaystyle \bold{(b)}\) If a sample of a different compound decomposes into \(\displaystyle 0.429\) g of carbon and \(\displaystyle 0.571\) g of oxygen, what is its ratio of the mass of \(\displaystyle \text{O}\) to \(\displaystyle \text{C}\)? \(\displaystyle \bold{(c)}\) According to Dalton’s atomic theory, what is the empirical formula of the second compound?

Why are you now posting Chemistry questions (along with a multitude of other inappropriate topic areas) in a Maths forum????

Is this you trying to get yourself elevated to "Elite" status?

I doubt if anyone will be impressed.

(I also doubt if the Chess Guy will be overly pleased at you purloining his image for your avatar. Can't you just use your own ugly mug? )

 

[pka]

A \(\displaystyle 1.0\)-g sample of carbon dioxide \(\displaystyle (\text{CO}_{2})\) is fully decomposed into its elements, yielding \(\displaystyle 0.273\) g of carbon and \(\displaystyle 0.727\) g of oxygen. \(\displaystyle \bold{(a)}\) What is the ratio of the mass of \(\displaystyle \text{O}\) to \(\displaystyle \text{C}\)? \(\displaystyle \bold{(b)}\) If a sample of a different compound decomposes into \(\displaystyle 0.429\) g of carbon and \(\displaystyle 0.571\) g of oxygen, what is its ratio of the mass of \(\displaystyle \text{O}\) to \(\displaystyle \text{C}\)? \(\displaystyle \bold{(c)}\) According to Dalton’s atomic theory, what is the empirical formula of the second compound?

Post that question here: https://chemistryhelpforum.com/community/

 

[logistic_guy]

\(\displaystyle \bold{(a)}\)

\(\displaystyle \frac{0.727}{0.273} = 2.66\)

 

[logistic_guy]

\(\displaystyle \bold{(b)}\)

\(\displaystyle \frac{0.571}{0.429} = 1.33\)

 

[logistic_guy]

\(\displaystyle \bold{(c)}\)

Dalton’s atomic theory depends on the ratio of moles of the two elements.

Let us calculate the moles of \(\displaystyle \text{Carbon}\).

\(\displaystyle \frac{0.429}{12.011} \approx 0.0357\)

Let us calculate the moles of \(\displaystyle \text{Oxygen}\).

\(\displaystyle \frac{0.571}{15.999} \approx 0.0357\)

The \(\displaystyle \text{ratio} = \frac{0.0357}{0.0357} = 1\)

This means that for every \(\displaystyle 1\) carbon atom, there is \(\displaystyle 1\) oxygen atom.

Therefore, the second compound must be \(\displaystyle \text{CO}\).