A SAMPLE OF 5.5L OF ARAGON DAS IS STORED IN A SYLINDER AT A TEMPERATURE OF 32.2C AND A PRESSURE 8.42 ATM. THE SAMPLE IS TRANSFERED COMPLETELY TO ANOTHER 2.8L CYLINDER. SEVERAL HOURS AFTER THE TRANSFER THE SECOND CYLINDER HAS OBTAINED A TEMPERATURE OF 60C. WHAT IS THE PRESSURE OF THE SECOND CYLINDER?

(P1V1)/T1 = (P2V2)/T2
Don't forget to change T to Kelvin.

To find the pressure of the second cylinder, we can use the combined gas law equation:

(P1 * V1) / T1 = (P2 * V2) / T2

Given:
P1 = 8.42 atm (pressure of the first cylinder)
V1 = 5.5L (volume of the first cylinder)
T1 = 32.2°C (temperature of the first cylinder)

V2 = 2.8L (volume of the second cylinder)
T2 = 60°C (temperature of the second cylinder)

First, we need to convert the temperatures to Kelvin since temperature must be in Kelvin in the gas law equation. The conversion from Celsius to Kelvin is done by adding 273.15 to the Celsius temperature.

T1 = 32.2°C + 273.15 = 305.35 K
T2 = 60°C + 273.15 = 333.15 K

Now let's substitute the values into the combined gas law equation:

(8.42 atm * 5.5L) / 305.35 K = (P2 * 2.8L) / 333.15 K

To solve for P2 (pressure of the second cylinder), we can cross-multiply and isolate P2:

(P2 * 2.8L) = (8.42 atm * 5.5L) * (333.15 K / 305.35 K)

(P2 * 2.8L) = (46.31 atm * L * K)

P2 = (46.31 atm * L * K) / 2.8L

P2 ≈ 165.39 atm

Therefore, the pressure of the second cylinder is approximately 165.39 atm.