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2 answers:
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Answer:
The density of CO₂ gas at 27 Celsius and 0.500 atm is 0.89
Explanation:
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:
<u><em>P*V = n*R*T Equation (A)</em></u>
where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas.
Density allows you to measure the amount of mass in a given volume of a substance. So density is defined as the quotient between the mass of a body and the volume it occupies:
Being the molar mass of a substance the mass contained in one mole of said substance, the number of moles can be expressed as:
<em>Equation (B)</em>
Replacing in <u><em>Equation (A)</em></u>:
P*V= *R*T
Solving to get the definition of density expressed in the equation, you get:
Being:
- P=0.500 atm
- Molar mass CO₂= 44 g/mole
- R= 0.082
- T= 27 C= 300 K (being 0 C=273 K)
and replacing:
you get:
density= 0.89
<em><u>The density of CO₂ gas at 27 Celsius and 0.500 atm is 0.89 </u></em><em><u></u></em>
Answer:
The answers are;
1. 8.2 liters
2. 1214.84 ml
3. 318.027 K
4. 4.00 l.
Explanation:
1. Boyle's law states that the volume of given mass of gas is inversely proportional to its pressure at constant temperature
that is
P₁·V₁ = P₂·V₂
Where:
P₁ = Initial pressure = 40.0 mm Hg
V₁ = Initial volume = 12.3 liters
P₂ = Final pressure = 60.0 mm Hg
V₂ = Final volume = Required
From P₁·V₁ = P₂·V₂, V₂ is given by
= 8.2 l
The volume reduces to V₂ = 8.2 liters
2. Here Charles law states that
T₁ = Initial temperature = 27.0 °C = 300.15 K
V₁ = Initial volume = 900.0 mL
T₂ = Final temperature = 132.0 °C = 405.15 K
V₂ = Final volume = Required
Therefore =
= 1214.84 ml
V₂ = 1214.84 ml
3. Gay-Lussac's Law states that
Where:
P₁ = Initial pressure = 15.0 atmospheres
T₁ = Initial temperature = 25.0 °C = 298.15 K
P₂ = Final pressure = 16.0 atmospheres
T₂ = Final temperature = Required
∴
= = 318.027 K
T₂ = 318.027 K
4. Avogadro's law states that,
Equal volume of all gases at the same temperature and pressure contain equal number of molecules.
Therefore if 5.00 moles of gas occupies 2.00 l volume, then
1 moles will occupy 2.00/5 l volume and
10 moles will occupy 2.00/5 × 10 or 4.00 l volume.