A 50.0 leader propane tank contains the gas at a pressure of 65.0 ATM at a temperature of 16°C if the fixed volume tank is heated by the Sun to 41°C what will the pressure of gas be inside the tank

Answer 1

To solve this problem, we can use the ideal gas law formula:

PV = nRT

where:
P = pressure of the gas
V = volume of the gas
n = number of moles of gas
R = ideal gas constant (0.0821 atm L/mol K)
T = temperature of the gas in Kelvin

First, we need to convert the temperatures from Celsius to Kelvin:
Initial temperature (T1) = 16°C + 273 = 289 K
Final temperature (T2) = 41°C + 273 = 314 K

We are also given that the volume of the tank is fixed, so we can consider V to be constant.

Using the formula P1/T1 = P2/T2 (since V is constant):
P1/289 = P2/314

Solving for P2:
P2 = P1 * 314 / 289
P2 = 65.0 ATM * 314 / 289
P2 ≈ 70.72 ATM

Therefore, the pressure of the gas inside the tank when heated to 41°C will be approximately 70.72 ATM.