When oxygen expands from the liquid to gaseous state how much more volume does it occupy?
I'm not sure exactly how the answer is to be expressed but we can make some good suggestions. Suppose we have exactly 1.00 mL oxygen liquid. The density of liquid oxygen at the boiling point (90.2 K) is 1.14 g/mL. If it vaporizes at this temperature it will become a gas and will occupy a volume determined by PV = nRT.
P = 1 atm
V = you calculate--remember the answer will be in liters, you can convert to mL by multiplying by 1000.
n = 1.14*1/32 = 0.0356 moles
R = 0.08206
T = 90.2
Post your work if you get stuck.
You can recalculate the volume at room temperature (25 C or 298 K) which will show an even larger increase.
When oxygen expands from the liquid to gaseous state, it undergoes a substantial increase in volume. To calculate the change in volume during this phase transition, you need to know the initial and final volume of the oxygen.
If we assume that the oxygen is at its boiling point of -183 degrees Celsius (or 90.15 Kelvin) when it transitions from liquid to gas, and considering the ideal gas law, we can determine the change in volume using the equation:
V2 = V1 * (T2 / T1)
Where:
V1 = Initial volume
T1 = Initial temperature
V2 = Final volume
T2 = Final temperature
For oxygen, we can use an estimate volume of 1 liter in its liquid state at its boiling point and assume it expands to its gaseous state at room temperature, around 298 Kelvin.
V2 = 1 liter * (298K / 90.15K)
V2 = 3.30 liters
Therefore, when oxygen expands from the liquid to gaseous state, it occupies approximately 3.30 times more volume.