Final answer:
There are 474.5 grams of chlorine gas in a 150-liter cylinder at 1.00 atm and 0 degrees Celsius, calculated using the ideal gas law and the molar mass of chlorine.
Step-by-step explanation:
To determine how many grams of chlorine gas are present in a 150-liter cylinder at 1.00 atm and 0 degrees Celsius, we can use the ideal gas law PV=nRT. Here, P represents the pressure of the gas, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
The ideal gas constant R is 0.0821 atm·L/mol·K, and the molar mass of chlorine (Cl2) is 70.906 g/mol. Since the conditions provided are at standard temperature and pressure (STP), where 1 mole of any ideal gas occupies 22.41 liters, we can straightforwardly calculate the moles of chlorine gas using the volume:
n = V / 22.41L = 150L / 22.41L/mol = 6.693 mol
Next, we calculate the mass of chlorine by multiplying the moles by the molar mass of Cl2:
Mass = n × molar mass = 6.693 mol × 70.906 g/mol = 474.5 grams
Therefore, there are 474.5 grams of chlorine gas in the 150-liter cylinder at 1.00 atm and 0 degrees Celsius.