At 517 mm Hg and 24 °C, a sample of gas occuples a volume of 95 ml. The gas is transferred to a 225-ml flask and the temperature
2 answers:
Answer:
Explanation:
Hello,
In this case, we employ the combined ideal gas law in order to understand the volume-gas-pressure behavior as shown below:
Hence, solving for the final pressure P2, we obtain (do not forget temperature must be absolute):
Best regards.
Answer:
195mmHg is the pressure of the flask
Explanation:
Combined gas law defines the relationship of pressure, absolute temperature and volume of a gas under different conditions. The formula is:
In the problem, initial conditions of the gas are:
517mmHg = P₁
24°C + 273.15 = 297.15K = T₁
95mL = V₁
And final conditions are:
225mL = V₂
8.0°C + 273.15 = 265.15K = T₂
Replacing:
P₂ = <em>195mmHg is the pressure of the flask</em>
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There are 3 parts in this question:
1) To find the initial Boyle's constant
2) To find the final Boyle's constant
3) To verify whether gas is obeying Boyle's law or not
Given data:
The initial volume of the cylinder(in litres) =
= 12.0 L
The initial pressure(in atmospheric pressure) =
= 4.0 atm
The final pressure(in atmospheric pressure) =
= 8.0 atm
The final volume of the cylinder(in litres) =
= 6.0 L
First you need to know what Boyle's law is:
<span>Boyle's law states that the pressure of a given mass of an ideal gas is inversely proportional to its volume at a constant temperature.
</span>
The Mathematical form of Boyle's law is:
Where,
P = Pressure
V = Volume of the gas
k = Boyle's constant
Now let's solve aforementioned parts one by one:
1.
The initial volume of the cylinder(in litres) = = 12.0 L
The initial pressure(in atmospheric pressure) = = 4.0 atm
The Boyle's constant = = ?
According to the Boyle's law,
=> = 
Plug-in the values in the above equation, you would get:
= 4.0 * 12.0 = 48
Ans-1) = 48
2.
The final pressure(in atmospheric pressure) = = 8.0 atm
The final volume of the cylinder(in litres) = = 6.0 L
The Boyle's constant = = ?
According to the Boyle's law,
=> = 
Plug-in the values in the above equation, you would get:
= 8.0 * 6.0 = 48
Ans-2) = 48
3.
In order to verify Boyle's law, the initial Boyle's constant should be EQUAL to the final Boyle's constant, meaning:
=
Since,
= 48
= 48
Therefore,
48=48.
Ans-3) Hence proved: The gas IS obeying the Boyle's law.
-i
1) To find the initial Boyle's constant
2) To find the final Boyle's constant
3) To verify whether gas is obeying Boyle's law or not
Given data:
The initial volume of the cylinder(in litres) =
The initial pressure(in atmospheric pressure) =
The final pressure(in atmospheric pressure) =
The final volume of the cylinder(in litres) =
First you need to know what Boyle's law is:
<span>Boyle's law states that the pressure of a given mass of an ideal gas is inversely proportional to its volume at a constant temperature.
</span>
The Mathematical form of Boyle's law is:
Where,
P = Pressure
V = Volume of the gas
k = Boyle's constant
Now let's solve aforementioned parts one by one:
1.
The initial volume of the cylinder(in litres) =
The initial pressure(in atmospheric pressure) =
The Boyle's constant =
According to the Boyle's law,
=>
Plug-in the values in the above equation, you would get:
Ans-1)
2.
The final pressure(in atmospheric pressure) =
The final volume of the cylinder(in litres) =
The Boyle's constant =
According to the Boyle's law,
=>
Plug-in the values in the above equation, you would get:
Ans-2)
3.
In order to verify Boyle's law, the initial Boyle's constant should be EQUAL to the final Boyle's constant, meaning:
Since,
Therefore,
48=48.
Ans-3) Hence proved: The gas IS obeying the Boyle's law.
-i