a 5.0-L flask contains 0.60 g 02 at a temperature off 22degrees C.what is the pressure (in atm) inside the flask?
Use PV = nRT
Ok but what is n??
To find the pressure inside the flask, we can use the ideal gas law equation, which states that:
PV = nRT
Where:
P is the pressure
V is the volume
n is the number of moles of gas
R is the ideal gas constant (0.0821 L·atm/(mol·K))
T is the temperature in Kelvin
Now, let's calculate the number of moles of oxygen (O2):
Convert the given mass of oxygen to moles using the molar mass of oxygen (O2), which is approximately 32 g/mol.
molar mass of O2 = 32 g/mol
moles of O2 = mass of O2 / molar mass of O2
= 0.60 g / 32 g/mol
≈ 0.018750 moles
We also need to convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
= 22 + 273.15
= 295.15 K
Now, we have the following known values:
V = 5.0 L (volume)
n = 0.018750 mol (moles of O2)
R = 0.0821 L·atm/(mol·K) (ideal gas constant)
T = 295.15 K (temperature in Kelvin)
Substituting these values into the ideal gas law equation:
PV = nRT
P * 5.0 L = 0.018750 mol * 0.0821 L·atm/(mol·K) * 295.15 K
P = (0.018750 mol * 0.0821 L·atm/(mol·K) * 295.15 K) / 5.0 L
P ≈ 0.217 atm
Therefore, the pressure inside the flask is approximately 0.217 atm.