A six-carbon organic compound containing oxygen is suspected of being either a secondary alcohol or a ketone. which chemical or
physical test would best distinguish between these two possibilities?
1 answer:
Following are the possible isomers of secondary alcohol and ketones for six carbon molecules. In order to distinguish between sec. alcohol and ketone we can simply treat the unknown compound with acidified Potassium Dichromate (VI) in the presence of acid. If with treatment with unknown compound the colour of K2Cr2O7 (potassium dichromate VI) changes from orange to green then it is confirmed that the unknown compound is sec. alcohol, or if no change in colour is detected then ketone is confirmed. This is because ketone can not be further oxidized while, sec. alcohol can be oxidized to ketones as shown below,
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<u>Answer:</u> The empirical and molecular formula of the compound is and
respectively
<u>Explanation:</u>
We are given:
Mass of C = 3.758 g
Mass of H = 0.316 g
Mass of O = 1.251 g
To formulate the empirical formula, we need to follow some steps:
- <u>Step 1:</u> Converting the given masses into moles.
Moles of Carbon =
Moles of Hydrogen =
Moles of Oxygen =
- <u>Step 2:</u> Calculating the mole ratio of the given elements.
For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.078 moles.
For Carbon =
For Hydrogen =
For Oxygen =
- <u>Step 3:</u> Taking the mole ratio as their subscripts.
The ratio of C : H : O = 4 : 4 : 1
The empirical formula for the given compound is
For determining the molecular formula, we need to determine the valency which is multiplied by each element to get the molecular formula.
The equation used to calculate the valency is:
We are given:
Mass of molecular formula = 130 g/mol
Mass of empirical formula = 68 g/mol
Putting values in above equation, we get:
Multiplying this valency by the subscript of every element of empirical formula, we get:
Hence, the empirical and molecular formula of the compound is and
respectively
Considering the definition of molarity and molar mass, the mass of NaF required is 3.771 grams.
<h3>Definition of molarity</h3>Molar concentration or molarity is a measure of the concentration of a solute in a solution and indicates the number of moles of solute that are dissolved in a given volume.
The molarity of a solution is calculated by dividing the moles of solute by the volume of the solution:
Molarity is expressed in units .
The molar mass of substance is a property defined as its mass per unit quantity of substance, in other words, molar mass is the amount of mass that a substance contains in one mole.
<h3 /><h3>Mass of NaF required</h3>In this case, you know:
- molarity= 0.15 M= 0.15
- number of moles= ?
- volume= 600 mL= 0.6 L
Replacing in the definition of molarity:
Solving:
0.15 × 0.6 L= number of moles
<u><em>0.09 moles= number of moles</em></u>
The molar mass of NaF is 41. 9 g/mol. So, you can apply the following rule of three: If by definition of molar mass 1 mole of the compound contains 41.9 grams, 0.09 moles of the compound contains how much mass?
<u><em>mass= 3.771 grams</em></u>
Finally, the mass of NaF required is 3.771 grams.
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