In what situation would boiling occur more rapidly?

Boiling occurs when a liquid's vapor pressure equals the external pressure surrounding it. In a vacuum environment, the external pressure is significantly reduced, often to the point where the vapor pressure of the liquid can reach that level at much lower temperatures than it typically would under normal atmospheric conditions. This allows the liquid to transition to a gas state more rapidly, resulting in quicker boiling.

In contrast, high barometric pressure would increase the boiling point of a liquid, meaning it would take longer for the liquid to boil. At sea level, pure substances boil at a standard temperature, but this is not necessarily faster than in a vacuum. Higher altitudes result in lower atmospheric pressure, which would decrease the boiling point, but boiling would still not occur as rapidly as it would in a vacuum where pressure is minimized significantly.