What is the volume at STP, in liters, occupied by 26.4 g of F2 gas?
Convert 26.4 g F2 to moles. moles = gfams/mola mass.
Then use PV = nRT. Don't forget to use T in Kelvin. Standard P is 1 atm and standard
T is 273 K. Solve for V ( in liters).
To find the volume of a gas at STP (Standard Temperature and Pressure), you can use the formula:
V = (n * R * T) / P
Where:
V = volume of the gas
n = number of moles of the gas
R = ideal gas constant (0.0821 L * atm / K * mol)
T = temperature of the gas in Kelvin
P = pressure of the gas in atmospheres
Since we have the mass of the gas, we need to convert it to moles before using the formula. The molar mass of F2 gas is 38 g/mol.
Step 1: Convert mass to moles
n = 26.4 g F2 * (1 mol F2 / 38 g F2)
n = 0.6947 mol F2
Step 2: Plug the values into the formula
V = (0.6947 mol * 0.0821 L * atm / K * mol * 273 K) / 1 atm
V = 16.11 L
Therefore, the volume occupied by 26.4 g of F2 gas at STP is 16.11 liters.
To find the volume of a gas at STP (Standard Temperature and Pressure), we can use the ideal gas law equation, which is:
PV = nRT
Where:
P = pressure (which is equal to 1 atm at STP)
V = volume in liters (what we are trying to find)
n = number of moles of the gas
R = ideal gas constant (0.08206 L·atm/mol·K)
T = temperature in Kelvin (which is 273.15 K at STP)
First, we need to calculate the number of moles of F2 gas using its molar mass.
The molar mass of F2 = 2 x atomic mass of fluorine
The atomic mass of fluorine = 19 g/mol
So, the molar mass of F2 = 2 x 19 = 38 g/mol
Now, we can find the number of moles of F2 gas:
number of moles (n) = mass (m) / molar mass (M)
n = 26.4 g / 38 g/mol
n ≈ 0.6947 mol (rounded to four decimal places)
Next, we can plug in the values into the ideal gas law equation:
PV = nRT
(1 atm) × V = (0.6947 mol) × (0.08206 L·atm/mol·K) × (273.15 K)
Now, solve for V:
V = (0.6947 mol × 0.08206 L·atm/mol·K × 273.15 K) / 1 atm
V ≈ 14.23 L (rounded to two decimal places)
Therefore, the volume occupied by 26.4 g of F2 gas at STP is approximately 14.23 liters.