Final answer:
The pressure of an ideal gas, we can use the ideal gas law equation PV = nRT. First, convert the volume from milliliters to liters and the temperature from Celsius to Kelvin. Then, plug the values into the ideal gas law equation and solve for pressure.
Step-by-step explanation:
To calculate the pressure of an ideal gas, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.
First, we need to convert the volume from milliliters to liters. Since 1 L = 1000 mL, the volume is 500 mL / 1000 = 0.5 L.
Next, we convert the temperature from Celsius to Kelvin. We add 273.15 to the Celsius temperature, so 23 °C + 273.15 = 296.15 K.
Now we can plug the values into the ideal gas law equation. P * 0.5 L = 2.2 moles * R * 296.15 K. Since R is a constant, we can rearrange the equation to solve for P: P = (2.2 moles * R * 296.15 K) / 0.5 L.
Let's assume the value of R is 0.08206 L * atm / (mol * K). Substituting this value in, we get P = (2.2 moles * 0.08206 L * atm / (mol * K) * 296.15 K) / 0.5 L = 199.267 atm.
Therefore, the pressure of the ideal gas is approximately 199.267 atm.