What is the number of molecules of c2h5oh in a 3m solution that contains 4.00kg h2o?

1 answer:

3 0

The number of C2H5OH in a 3 m solution that contain 4.00kg H2O is calculate as below

M = moles of the solute/Kg of water

that is 3M = moles of solute/ 4 Kg
multiply both side by 4

moles of the solute is therefore = 12 moles

by use of Avogadro law constant

1 mole =6.02 x10^23 molecules

what about 12 moles

=12 moles/1 moles x 6.02 x10^23 = 7.224 x10^24 molecules

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What is the differences between amorphous solid and crystalline solid

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Answer:

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A compound is found to contain 11.21 % hydrogen and 88.79 % oxygen by mass. What is the empirical formula for this compound?

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Answer:

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Explanation:

The empirical formular of the compound is obtained using the following steps;

Step 1: Divide the percentage composition by the atomic mass

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Oxygen = 88.79 / 16 = 5.55

Step 2: Divide by the lowest number

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Boyle’s law states that the volume of a gas is inversely proportional to its pressure if the

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Boyle's law states that the volume of a fixed mass of a gas is inversely proportional to its temperature if<u> the temperature and the number of particles are constant.</u>

<h3>Further Explanation</h3><h3>Boyles’s law </h3>

This gas law states that the volume of a fixed mass of a gas is inversely proportional to its pressure at constant absolute temperature.
Therefore, when the volume of an ideal gas is increased at constant temperature then the pressure of the gas will also increase.
Mathematically; Volume α 1/Pressure

Vα1/P

Therefore, constant k, is = PV

<h3>Other gas Laws</h3><h3>Gay-Lussac’s law </h3>

It states that at constant volume, the pressure of an ideal gas I directly proportional to its absolute temperature.
Thus, an increase in pressure of an ideal gas at constant volume will result to an increase in the absolute temperature.

<h3>Charles’s law</h3>

It states that the volume of a fixed mass of a gas is directly proportional to absolute temperature at constant pressure.
Therefore, an increase in volume of an ideal gas causes a corresponding increase in its absolute temperature and vice versa while the pressure is held constant.

<h3>Dalton’s law </h3>

It is also known as the Dalton’s law of partial pressure. It states that the total pressure of a mixture of gases is always equivalent to the total sum of the partial pressures of individual component gases.
Partial pressure refers to the pressure of an individual gas if it occupies the same volume as the mixture of gases.

Keywords: Gas law, Boyles's law, pressure, volume, absolute temperature, ideal gas

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