To solve this problem, we can use the ideal gas law, which states:
PV = nRT
Where: P is the pressure V is the volume n is the number of moles of gas R is the ideal gas constant T is the temperature in Kelvin
First, let's convert the initial temperature from Celsius to Kelvin:
T1 = 25°C + 273.15 = 298.15 K
We can rearrange the ideal gas law equation to solve for the final pressure:
P2 = (P1 * T2) / T1
Where: P1 is the initial pressure T2 is the final temperature in Kelvin T1 is the initial temperature in Kelvin P2 is the final pressure (what we're trying to find)
Now, let's calculate the final temperature:
T2 = 3 * T1 = 3 * 298.15 K = 894.45 K
Plugging in the values into the equation:
P2 = (600 atm * 894.45 K) / 298.15 K P2 = 1791 atm (rounded to three significant figures)
Therefore, if the temperature is tripled, the pressure of the helium tank will be approximately 1791 atm.