Synthetic diamonds can be manufactured at pressures of #6.00 times 10^4# atm. If we took 2.00 liters of gas at 1.00 atm and compressed it to a pressure #6.00 times 10^4# atm, what would the volume of that gas be?
The volume is
Apply Boyle's Law
The temperature being constant
The initial volume is
The initial pressure
The final pressure is
The final volume is
Rather small, a fraction of a millilitre….
Old Boyle's Law insists that
And so …………….
And note our assumptions...we ASSUME (perhaps wrongly) that the gas would not undergo a phase change.
Assuming gas is ideal undergoing a constant temperature process then
According to Boyle's Law, at constant temperature
As per given data, initial pressure
The final volume of gas becomes