0.5 mol CCl4 is introduced into a 10.0L flask.what fraction of the total volume of the
flask is occupied by CCl4 molecules?
To determine the fraction of the total volume occupied by CCl4 molecules, we need to calculate the volume of the CCl4 molecules and divide it by the total volume of the flask.
First, we need to convert the given amount of CCl4 in moles into the volume using the ideal gas law:
PV = nRT,
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.
Since we are given the number of moles (0.5 mol), we can rearrange the formula as:
V = (nRT) / P,
assuming constant pressure and temperature.
The ideal gas constant R is 0.0821 L·atm/(mol·K) and the standard temperature and pressure (STP) conditions are 0 °C (273.15 K) and 1 atm respectively. However, the given problem does not specify the temperature and pressure conditions. Thus, we need additional information to calculate the exact volume.
Once we know the volume of the CCl4 molecules, we can divide it by the total volume of the flask (10.0 L) to find the fraction occupied by CCl4 molecules.
In summary, to find the fraction of the total volume occupied by CCl4 molecules, we need to know the temperature and pressure conditions.