A sample of O2 inside a container is measured and found to have a volume of 15 L, a mass of 16.0 g, and a temperature of 273 K. What can we say about the pressure of the gas, P? Hint: Don't forget that the molar volume of an ideal gas at STP is 22.4 L (Figure 10.8).
To find the pressure of the gas, we can use the ideal gas equation:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to calculate the number of moles of O2 in the sample. We can do this using the molar mass of O2, which is 32 g/mol (16 g for each O atom):
n = mass / molar mass
n = 16.0 g / 32 g/mol
n = 0.5 moles
Next, we can rearrange the ideal gas equation to solve for pressure:
P = (nRT) / V
P = (0.5 moles)(0.0821 L∙atm/mol∙K)(273 K) / 15 L
P = 0.5 * 0.0821 * 273 / 15 atm
P = 0.750 atm
Therefore, the pressure of the gas inside the container is 0.75 atm.