Answer :
The pressure of a 5.00 L tank containing 2.50 moles of oxygen at 39.3 °C is calculated using the Ideal Gas Law and is found to be 1.288 atm.
To determine the pressure in atm of a 5.00 L tank with 2.50 moles of oxygen at 39.3 °C, we can use the Ideal Gas Law, which is PV = nRT, where P is the pressure in atmospheres (atm), V is the volume in liters (L), n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin. The first step is to convert the temperature from degrees Celsius to Kelvin by adding 273.15 to the Celsius temperature. We have T = 39.3 + 273.15 = 312.45 K.
Now, we can solve for P (pressure) using the Ideal Gas Law equation:
Convert the given temperature to Kelvin: T(K) = 39.3 °C + 273.15 = 312.45 K
Use the Ideal Gas Law: PV = nRT
Substitute the known values (using R = 0.0821 L·atm/mol·k): P(5.00 L) = 2.50 mol × 0.0821 L·atm/mol·k × 312.45 K
Solve for P: P = (2.50 mol × 0.0821 L·atm/mol·k × 312.45 K) / 5.00 L
Calculate P: P = 1.288 atm (rounded to three significant figures)
The pressure of the gas in the tank is 1.288 atm.
