[TextClick]

Synthetic diamonds can be manufactured at pressures of 6.00 x 10^4 atm. If we took 2.00 liters of gas at 1.00 atm and compressed it to a pressure of 6.00 x 10^4 atm, at constant temperature, what would the volume of that gas be?

[billnotgatez]

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Hint you might start with the Ideal Gas Law
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[AWK]

In some ways, this is a nonsense problem.
At this pressure at a temperature of around 3000-3500 K, you can actually get synthetic diamonds by HPHT method. But even under standard temperature conditions at such pressure, the ideal gas equation does not apply to any real gas, e.g. the volume of helium (most similar to ideal gas) when changing pressure from 100 to 500 atm (note - the pressure is 12 times lower than given by you) at 100 K decreases volume 3.4 times instead of 5 times and at 600 K - 4.6 times respectively.
At higher pressures, these deviations from ideal gas behavior will be even greater.

[Enthalpy]

In some ways, this is a nonsense problem.

I don't even see any way this problem could make sense. The volume depends fundamentally on the size and nature of the molecules that make up the gas, so "2L of gas" lacks data. "At constant temperature" is strictly insufficient too.

I made springs that compress a liquid at a few 1000 bar, the volume shrinks by 10-30%. Even the liquid's volume at 1atm doesn't tell the volume at 60 000 bar.

The way this problem is formulated suggests to use the ideal gas law, which cannot apply here. Bad luck.