What is the mass of oxygen in a ml flask if the pressure is 1.00 atm and a temperature of 22.0 Celsius?
WHAT mL flask.
Use PV = nRT. Don't forget to use T in Kelvin. Also, convert mL to L and use P in atmospheres.
Julie, check your 2-6-11,5:49pm post.
To determine the mass of oxygen in a flask, we can use the ideal gas law equation:
PV = nRT
where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
First, we need to convert the given temperature in Celsius to Kelvin:
T(K) = T(°C) + 273.15
Given:
P = 1.00 atm
T = 22.0 °C
Converting temperature to Kelvin:
T(K) = 22.0 + 273.15 = 295.15 K
Now, we need to know the volume of the flask. You mentioned it as a "ml flask," so let's assume a volume of 1 ml. However, it's important to note that the volume should be in liters to be consistent with the units of the ideal gas constant.
Converting volume to liters:
V(L) = V(ml) / 1000
Given:
V = 1 ml = 1/1000 L = 0.001 L
Now, let's rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT
Substituting the given values:
n = (1.00 atm * 0.001 L) / (0.0821 L·atm/(mol·K) * 295.15 K)
Now, we can calculate the number of moles (n) of oxygen in the flask.
Finally, to determine the mass of oxygen, we need to know the molar mass of oxygen, which is approximately 32.00 g/mol.
To calculate the mass of oxygen:
mass = n * molar mass
Substituting the calculated value of n and the molar mass of oxygen:
mass = n * 32.00 g/mol
By following these steps and substituting the given values, you can calculate the mass of oxygen in the flask.