calculate the mass of chlorine gas contained in a 5dm3 flask at 25degrees celsuis and 98kpa pressure.
To calculate the mass of chlorine gas contained in the flask, you need to use the ideal gas law equation, which relates the pressure (P), volume (V), temperature (T), and number of moles (n) of a gas.
The ideal gas law equation is as follows:
PV = nRT
Where:
P = pressure (in Pa)
V = volume (in m^3)
n = number of moles
R = gas constant (8.314 J/(mol·K))
T = temperature (in Kelvin)
First, let's convert the given values into the appropriate units:
Volume: 5 dm^3 = 5 × 10^-3 m^3 (since 1 dm^3 = 10^-3 m^3)
Temperature: 25 degrees Celsius = 25 + 273 = 298 K (since 0 degrees Celsius is equal to 273 K)
Pressure: 98 kPa = 98,000 Pa (since 1 kPa = 1000 Pa)
Now, we can rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT
Substituting the given values:
n = (98,000 Pa) × (5 × 10^-3 m^3) / ((8.314 J/(mol·K)) × 298 K)
Calculating this expression will give the number of moles of chlorine gas in the flask.
Once you have the number of moles, you can calculate the mass of chlorine gas using the molar mass of chlorine (Cl₂), which is approximately 70.90 g/mol.
Mass = number of moles × molar mass
Simply multiply the number of moles by the molar mass to get the mass of chlorine gas in grams.