A 5.0 L flask contains 0.60 g of O2 at a temperature of 22°C. What is the pressure inside the flask?

To find the pressure of the O_2 gas inside the 5.0 L flask, we can use the Ideal Gas Law, which is stated as:

PV = nRT

Where:

P is the pressure of the gas, V is the volume of the gas, n is the number of moles of the gas, R is the ideal gas constant, T is the temperature of the gas in Kelvin.

First, let's convert the given values to the proper units for applying the Ideal Gas Law.

You're given: - Mass (m) of O_2 = 0.60 g - Volume (V) of the flask = 5.0 L (which is already in liters) - Temperature (T) = 22°C

To convert temperature into Kelvin: T(K) = T(°C) + 273.15 T(K) = 22 + 273.15 T(K) = 295.15 K

Next, we calculate the number of moles (n) of O_2. The molar mass of oxygen (O) is 16.00 g/mol, but since O_2 is a diatomic molecule, its molar mass is 2 * 16.00 g/mol = 32.00 g/mol.

n = m / Molar mass n = 0.60 g / 32.00 g/mol n = 0.01875 mol

The gas constant (R) value when using the pressure in atmospheres (atm) and volume in liters (L) is typically 0.0821 (L·atm)/(K·mol).

Now we can find the pressure (P).

PV = nRT

P = nRT / V P = (0.01875 mol) * (0.0821 L·atm/K·mol) * (295.15 K) / (5.0 L)

P = (0.01875 * 0.0821 * 295.15) / 5.0

P = (0.0015397125 * 295.15) / 5.0

P = 0.45409902375 / 5.0

P = 0.09082 atm

So, the pressure inside the 5.0 L flask containing 0.60 g of O2 at a temperature of 22°C is approximately 0.09082 atm.