A 1.0 L tank can explode if the pressure exceeds 12.5 atm. At 25 degrees Celsius, the gas inside the tank is at a pressure of 2.07 atm. To what temperature can the tank be heated before it may explode? (My answer was 151C, but im not positive). Please explain. Thanks!
2006-10-21 11:58:38 · 2 answers · asked by *AH AH* 1 in Science & Mathematics ➔ Chemistry
Previous answer is correct, based on ideal gas law:
PV=nRT
V, n and R are constant therefore
P (absolute pressure) is proportional to T (absolute temperature)
It is of course an interesting sort of tank which could withstand this temperature.
2006-10-21 13:40:23 · answer #1 · answered by Robert A 5 · 0⤊ 0⤋
that is a Gay - Lussac gas law.
the formula:
P1/T1 = P2/T2
*first you must convert the Celsius to Kelvin..
25 + 273 = 298 K
...then substitute the given to the equation
2.07atm / 298 K = 12.5 atm / T2
T2 = 1799.517 K
*converting it to Celsius
1799.517 - 273 = 1526.517 degrees Celsius
* the answer is, the gas tank will explode if the temperature exceeds 1526.517 degrees Celsius
...the Gay-Lussac's Law explains that pressure increases as temperature increases... if you will think about the pressure cooker, that is one of the applications of the law. According to your problem, the tank has a constant volume of 1 L, and if the pressure exceeds 12.5 atm it will explode. If you will analyze the problem, the first pressure that is given is 2.07 atm at 25 Celsius (you must convert the Celsius scale first to Kelvin), then using the reference data 12.5 atm, the second temperature is not given... applying the formula that I have stated above, you will get T2... since the P2 is more than P1, the temperature will definitely increase.
2006-10-21 19:16:17 · answer #2 · answered by jHorny-sHorny 2 · 0⤊ 0⤋