one litre of liquid methanol will occupy how much volume in the state of vapour at 60 deg. Celsius?
To determine the volume of one liter of liquid methanol in the vapor state at 60 degrees Celsius, we need to consider the properties of methanol and its vapor pressure.
First, we need to find the vapor pressure of methanol at 60 degrees Celsius. One way to obtain this information is by referring to a vapor pressure-temperature chart for methanol. Such charts provide the vapor pressure of a substance at various temperatures.
Once we know the vapor pressure of methanol at 60 degrees Celsius, we can use the ideal gas law to estimate the volume of the vapor. The ideal gas law equation is:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature in Kelvin
To convert Celsius to Kelvin, we can use the equation:
T(K) = T(°C) + 273.15
Assuming we have one mole of methanol, we can rearrange the ideal gas law equation to solve for V:
V = (nRT) / P
By substituting the values we have - the number of moles (n) as 1, the ideal gas constant (R), as well as the vapor pressure of methanol at 60 degrees Celsius (P), and the temperature converted to Kelvin (T) - we can calculate the volume (V) of methanol vapor.
Please note that the actual volume may not precisely match the calculated value due to various factors, such as non-ideal behavior of the methanol vapor or the presence of impurities.