If 0.278g of argon dissolves in 1.5 l of water at 62 bar, what quantity of argon will dissolve at 78 bar
1 answer:
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The molar mass of gas = 206.36 g/mol
<h3>Further explanation</h3>In general, the gas equation can be written
where
P = pressure, atm
V = volume, liter
n = number of moles
R = gas constant = 0.082 l.atm / mol K
T = temperature, Kelvin
mass (m)= 2.89 g
volume(V) = 346 ml = 0.346 L
T = 28.3 C + 273 = 301.3 K
P = 760 mmHg=1 atm
The molar mass (M) :
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