# Chemistry

Determine a possible Lewis Structure for each of the two compounds X and Y, given the following information:
Compound X contains only carbon, hydrogen, and oxygen. It is heated in a 1.00 liter flask to 160. degrees C and 1.00 atm until all of it has vaporized and fills the container completely. The flask is then cooled and found to contain 3.267 grams of compound X.
When 0.500 grams of compound X is burned in the presence of oxygen, 0.465 grams of water and 1.136 grams of CO2 are produced.
Compound X can be formed from the reaction of compound Y with potassium dichromate. Also, compound X can be neutralized by sodium hydroxide.

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1. So I'm thinking to start with the PV=nRT with the given pressure, volume, and temperature then find how many moles there are in compound X. After that divide the given mass of the compound (3.267 grams) by the calculated number of moles to find the molar mass of the compound X. I am stuck here, what do I do next?

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2. What's you have suggested sounds OK to me. That will give you the molar mass.

The second part (with 0.500 g X) lets you calculate the empirical formula.
1, Convert the CO2 to grams C.
2. Convert the H2O to grams H.
3 Grams O = 0.500 g - g C - g H = ?

Now convert g C, H, O to mols each and find the ratio of C, H, and O. That gives the empirical formula and together with part 1 gives the molecular formula.

The neutralization with NaOH suggests a carboxylic acid to me.
The Y + dichormate suggests an aldehyde (Y) being oxidized to an acid (X)

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posted by DrBob222

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