How many molecules are in 5.2L of carbon dioxide gas?
a mole of ANY gas occupies 22.4 L at stp
(5.2 / 22.4) * Avogadro's number
To determine the number of molecules in 5.2L of carbon dioxide gas, we need to apply the ideal gas law equation, which is:
PV = nRT
Where:
P is the pressure of the gas (in atm)
V is the volume of the gas (in liters)
n is the number of moles of gas
R is the ideal gas constant (0.0821 L·atm/mol·K)
T is the temperature of the gas (in Kelvin)
Since we want to find the number of molecules, we need to rearrange the equation to solve for n:
n = PV / RT
Now, we need to gather the values needed for the equation. The pressure (P) and temperature (T) are not provided in the question, so we'll assume standard temperature and pressure (STP), which is 1 atm and 273.15K, respectively.
The volume (V) given is 5.2L, and the ideal gas constant (R) is 0.0821 L·atm/mol·K.
Plugging these values into the equation:
n = (1 atm) * (5.2 L) / (0.0821 L·atm/mol·K * 273.15 K)
n ≈ 0.23 mol
To convert moles to molecules, we use Avogadro's number, which is approximately 6.022 × 10^23 molecules/mol.
n = (0.23 mol) * (6.022 × 10^23 molecules/mol)
n ≈ 1.3866 × 10^23 molecules
Therefore, there are approximately 1.3866 × 10^23 molecules in 5.2L of carbon dioxide gas.