Question

If fluorine gas (F₂) occupies a volume of 45.5 L at a pressure of 850
mmHg and a temperature of 100.0°C, what is the mass of fluorine gas
(F₂)?

Answer 1

Taking into account about the ideal gas law, the mass of fluorine gas is 63.2244 grams.

What is ideal gas law

An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P×V = n×R×T

where:

• P is the gas pressure.
• V is the volume that occupies.
• T is its temperature. The universal constant of ideal gases R has the same value for all gaseous substances.
• R is the ideal gas constant.
• n is the number of moles of the gas.

Definition of molar mass

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.

Mass of fluorine gas

In this case, you know:

• P= 850 mmHg= 1.11842 atm (being 1 mmHg= 0.00131579 atm)
• V= 45.5 L
• T =100 °C= 373 K (being 0°C= 273 K)
• R= 0.082 $\frac{atm L}{mol K}$
• n= ?

Replacing in the ideal gas law:

1.11842 atm ×45.5 L = n×0.082 $\frac{atm L}{mol K}$× 373 K

Solving:

n= (1.11842 atm ×45.5 L)÷ (0.082 $\frac{atm L}{mol K}$× 373 K)

n= 1.6638 moles

The molar mass of F₂ is 38 g/mole. Then you can apply the folowing rule of three: If by definition of molar mass 1 mole of the compound contains 38 grams, 1.6638 moles of the compound contains how much mass?

$mass= \frac{1.6638 molesx38 grams}{1 mole}$

mass= 63.2244 grams

Finally, the mass of fluorine gas is 63.2244 grams.

Learn more about

the ideal gas law:

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molar mass:

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brainly.com/question/17249726

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