Answer:
To calculate the pressure exerted by one mole of CO2 gas at 40 degrees Celsius, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (in Pascal or Pa)
V = Volume (in cubic meters or m^3)
n = Number of moles
R = Ideal gas constant (8.314 J/(mol·K))
T = Temperature (in Kelvin or K)
First, we need to convert the given volume from liters to cubic meters:
0.382 L = 0.382 × 10^(-3) m^3
Next, we need to convert the given temperature from degrees Celsius to Kelvin:
40 degrees Celsius = 40 + 273.15 K
Now, we can substitute the values into the ideal gas law equation:
P × 0.382 × 10^(-3) = 1 × 8.314 × (40 + 273.15)
Simplifying the equation:
P × 0.382 × 10^(-3) = 8.314 × 313.15
Dividing both sides by 0.382 × 10^(-3):
P = (8.314 × 313.15) / (0.382 × 10^(-3))
Calculating the pressure:
P ≈ 68,086 Pa
Therefore, the pressure exerted by one mole of CO2 gas at 40 degrees Celsius assuming ideal behavior is approximately 68,086 Pascal (Pa).
