Final answer:
To find the pressure of the gas, convert the temperature to Kelvin and use the ideal gas law. For 0.592 mol of an ideal gas at 22.3°C in a 4.0 L container, the pressure is approximately 3.66 atm.
Step-by-step explanation:
To calculate the pressure of a gas in a container, we can use the ideal gas law, which is PV = nRT, where P is pressure, V is volume, n is the amount of substance in moles, R is the ideal gas constant, and T is the temperature in Kelvin.
To solve the problem: A 4.0 L container holds 0.592 mol of an ideal gas at a temperature of 22.3 Celsius degrees, we first convert the temperature to Kelvin by adding 273.15 to the Celsius temperature.
So,T = 22.3 + 273.15 = 295.45 K.
Next, we use the ideal gas constant R = 0.0821 L·atm/(K·mol). Now we can solve for P:
P = (nRT)/V
P = (0.592 moles × 0.0821 L·atm/(K·mol) × 295.45 K) / 4.0 L
P ≈ 3.66 atm
Therefore, the pressure of the gas in the container is approximately 3.66 atm.