Answer:
4.7K
Explanation:
Given parameters:
Initial volume = 75L
Initial pressure = 125psi
to atm gives 8.5atm
Initial temperature = 288K
New volume = 6.1L
New pressure = 25psi
to atm gives 1.7atm
Unknown:
New temperature = ?
Solution:
To solve this problem, we use the combined gas law which is given below:
=
P, V and T are pressure, volume and temperature
1 and 2 are initial and new states
=
T2 = 4.7K
The volume increased to 0.64 L on increasing the temperature to boiling point of water.
<u>Explanation:</u>
One of the important laws used for understanding the kinetics of gas particles is Charle's law. It states that the volume occupied by gas molecules will be directly proportional to the Kelvin temperature of the molecules at constant pressure.
Volume ∝ Kelvin Temperature at constant Pressure
So, in this case, the initial volume of the container in which Nitrogen gas is kept is given as 0.5 L and the initial temperature of the Nitrogen gas is said to be 18°C.
Now the container is heated to boiling point of water which is 100°C, then the volume occupied by the gas should increase as per Charle's law.
Since here V₁ = 0.5 L
T₁ = 18°C = 18 + 273.15 = 291.15 K
T₂ = 100°C = 100 + 273.15 = 373.15 K
Thus, the volume increased to 0.64 L on increasing the temperature to boiling point of water.