Answer:
To calculate the mass of carbon dioxide gas (CO2) occupying 11.2 dm³ at 27°C and 10 kPa pressure, you can use the ideal gas law equation:
PV = nRT
Where: P = pressure (in Pa) V = volume (in m³) n = number of moles R = ideal gas constant (8.314 J/(mol·K)) T = temperature (in Kelvin)
First, convert the given values to the appropriate units: Volume (V) = 11.2 dm³ = 11.2 x 10^-3 m³ Pressure (P) = 10 kPa = 10,000 Pa Temperature (T) = 27°C = 27 + 273 = 300 K
Now, rearrange the ideal gas law equation to solve for n (number of moles): n = PV / RT
Substitute the given values into the equation and calculate the number of moles (n). Once you have the number of moles, you can calculate the mass of CO2 using the molar mass of CO2 (44.01 g/mol). The mass (m) is given by: m = n * M
Where: n = number of moles M = molar mass of CO2
By substituting the calculated value of n and the molar mass of CO2, you will obtain the mass of CO2 gas.
