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3 years ago

NEED HELP ASAP!!!

Chemistry

1 answer:

Alexxx [7]3 years ago

6 0

At room temperature oxygen, $O_2$ is present in the gas phase.

A gas is defined as a substance which is characterized by the rapidly movement of molecules which are widely separated. The shape and volume of gas is not definite that is they take on the shape of the container in which it is placed. The gas molecules have minimum inter-nuclear attractions and thus have high kinetic energy.

Thus, the sentences that describes oxygen at room temperature are:

It has no definite volume and takes the shape of its container.
Its particles move fast enough to overcome the attraction between them.
It has more energy than it would be at a cooler temperature as the kinetic energy is directly proportional to the temperature that is kinetic energy increases on increasing the temperature.

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A 35.161 mg sample of a chemical known to contain only carbon, hydrogen, sulfur, and oxygen is put into a combustion analysis ap

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Answer:

The empirical formulae is C6H12S02

Explanation:

1. First we need to obtain the mass of each element in the sample and compound formed

Carbon = (62.637 mg * 12.011 g/mol / 44.009 g/mol) = 17.094 mg of Carbon

Hydrogen = ( 25.641 mg * (2 *1..008 g/mol) / 18.015 g/mol) = 2.869 mg of Hydrogen

Sulphur = (13.54 mg * 32.066 g/mol / 64.066 g/mol) = 6.777 mg of Sulphur

2. Next is to determine the percentage composition. Here we divide the respective mass by the mass of the sample

Carbon = 17.094 / 35.161 * 100 = 48.62 %

Hydrogen = 2.869/ 35.161 *100 = 8.16 %

Sulphur = 6.777/ 31.321 *100 = 21.64 %

Oxygen = (100 - (48.62 + 8.16 + 21.64)) = 21.58 %

3. Next is to divide the mass assuming there are 100 mg by the respective atomic masses to obtain the number of moles

Carbon = 48.62 / 12.011 = 4.048 mol

Hydrogen = 8.16 / 1.008 = 8.095 mol

Sulphur = 21.64 / 32.066 = 0.675 mol

Oxygen = 21.58 / 16.000 = 1.348 mol

Next is to divide by the smallest value

Carbon = 4.048/ 0.675 =5.997 = 6

Hydrogen = 8.095 / 0.675 =11.993 =12

Sulphur = 0.675/ 0.675 = 1

Oxygen = 1.348 / 0.675 = 1.997 = 2

So therefore the empirical formulae of the sample is C6H12SO2

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