To determine the volume occupied by a given amount of gas, we can use the ideal gas law equation:
PV = nRT
Where: P = pressure (in atmospheres) V = volume (in liters) n = number of moles of gas R = ideal gas constant (0.0821 L·atm/(mol·K)) T = temperature (in Kelvin)
First, let's convert the given values to the appropriate units: Mass of O2 = 5.03g Temperature = 28°C = 28 + 273.15 = 301.15K Pressure = 0.998 ATM
Next, we need to determine the number of moles (n) of O2. To do this, we'll use the molar mass of oxygen gas (O2), which is approximately 32 g/mol.
n = mass / molar mass n = 5.03g / 32 g/mol ≈ 0.1573 mol
Now we can substitute the values into the ideal gas law equation and solve for the volume (V):
PV = nRT V = (nRT) / P
V = (0.1573 mol * 0.0821 L·atm/(mol·K) * 301.15K) / 0.998 ATM
Calculating the expression:
V ≈ 4.71 L
Therefore, approximately 5.03 grams of O2 at 28 degrees Celsius and a pressure of 0.998 ATM occupy a volume of around 4.71 liters.