A tank of chlorine gas contains 25.00 kg of pressurized liquid chlorine. If all the chlorine is released in its gaseous for at 17'C and 0.98atm, what volume does it occupy?
PV = nRT. You don't have n but n = grams/molar mass.
I got 1.7*10^4L but not sure if I was correct or not
I figured it out thanks for your help :D
To find the volume occupied by the chlorine gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure of the gas (in atm)
V = Volume of the gas (in liters)
n = Number of moles of gas
R = Ideal gas constant (0.0821 L·atm/(mol·K))
T = Temperature of the gas (in Kelvin)
To solve for the volume (V), we need to know the pressure (P), temperature (T), and the number of moles (n) of chlorine gas.
Given:
Pressure (P) = 0.98 atm
Temperature (T) = 17°C
First, we need to convert the temperature from Celsius to Kelvin.
T(K) = T(°C) + 273.15
T(K) = 17 + 273.15 = 290.15 K
Now, we need to find the number of moles of chlorine gas (n). To do this, we can use the molar mass of chlorine (Cl₂), which is 70.906 g/mol.
To find the number of moles, we can use the formula:
n = mass / molar mass
Given:
Mass of chlorine = 25.00 kg = 25000 g
Molar mass of chlorine (Cl₂) = 70.906 g/mol
n = 25000 g / 70.906 g/mol
n ≈ 352.16 mol
Now that we have the pressure (P = 0.98 atm), temperature (T = 290.15 K), and number of moles (n ≈ 352.16 mol), we can substitute these values into the ideal gas law equation:
PV = nRT
V = (nRT) / P
V = (352.16 mol) * (0.0821 L·atm/(mol·K)) * (290.15 K) / (0.98 atm)
Simplifying this equation will give us the volume (V) in liters.
V ≈ 11502.77 L
Therefore, the chlorine gas will occupy approximately 11502.77 liters.