A student has a 1g sample of each of the following compounds: NaCl, KBr, and KCL Which of the following lists the samples in ord
1 answer:
Given :
A student has a 1 g sample of each of the following compounds: NaCl, KBr, and KCl.
To Find :
The samples in order of increasing number of moles in the sample.
Solution :
Molecular mass of NaCl, KBr, and KCl is 58.5 g/mol , 119 g/mol and
74.5 g/mol respectively .
Moles of NaCl , .
Moles of KBr , .
Moles of KCl , .
The order of moles in increasing order is :
KBr , KCl and NaCl .
Hence , this is the required solution .
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Answer: 0.0007 moles of is released when temperature is raised.
Explanation:
To calculate the number of moles, we use the ideal gas equation, which is:
where,
P = pressure of the gas = 1.01 bar
V = Volume of the gas = 1L
R = Gas constant =
- Number of moles when T = 20° C
Temperature of the gas = 20° C = (273 + 20)K = 293K
Putting values in above equation, we get:
- Number of moles when T = 25° C
Temperature of the gas = 25° C = (273 + 25)K = 298K
Putting values in above equation, we get:
- Number of moles released =
Hence, 0.0007 moles of is released when temperature is raised from 20° C to 25° C
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