What is the volume at STP, in liters, occupied by 26.4 g of F2 gas?
Convert 26.4 g F2 to moles, substitute into PV = nRT and solve for V.
To determine the volume at STP (standard temperature and pressure) occupied by 26.4 g of F2 gas, we need to use the ideal gas law, which describes the relationship between pressure (P), volume (V), temperature (T), and the number of moles of gas (n).
The ideal gas law equation is:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
To solve for V, we need to rearrange the equation as follows:
V = (nRT) / P
Now, let's calculate the number of moles of F2 gas (n) using the molar mass (MM) of F2:
MM of F2 = 2 * atomic mass of F (fluorine)
= 2 * 19.00 g/mol
= 38.00 g/mol
n = mass / MM
= 26.4 g / 38.00 g/mol
= 0.69474 mol (rounded to five decimal places)
Next, we substitute the given values into the equation:
V = (nRT) / P
= (0.69474 mol * 0.0821 L·atm/(mol·K) * 273.15 K) / 1 atm
≈ 16.02 L (rounded to two decimal places)
Therefore, the volume occupied by 26.4 g of F2 gas at STP is approximately 16.02 liters.