2 Second Chemistry Question

 

Trying to theoretically boil 1 L of water in a closed container at 90 degrees Celsius and using the correlating boiling pressure for water at this temperature. In order to find the size of the container I tried using the Ideal Gas Law with the following variables:

 

V = solving for this.

P = .697 atm

n = 55.6 moles/liter

R = .0821 (L*atm)/(mol*K)

T = 363.15 K

 

The result shows a volume of 2378.3 L needed to carry out this experiment. I believe I have made a mistake. Surely water could be boiled in a smaller vessel, right?

you are assuming all of the water is gaseous. If it is all gaseous, then yes, you will want 2378.3L to contain that much steam at that temperature and pressure. However, the pressure will change as the water boils. Boiling anything inside a closed container can be extremely dangerous because of the high pressures built up. I hope you know what you're doing.