Question

If the vapor pressures of pure ethyl and diethyl are 0.08 and 0.7, calculate the pressure inside a can that contains 50g alcohol (46.1 g/mol) and 40 g diethyl (74.1 g/mol)

Answer 1

To calculate the pressure inside the can, we can use Raoult's law. By calculating the mole fractions of ethyl alcohol and diethyl, we can find the total pressure inside the can. The pressure inside the can is 0.346 atmospheres.

Step-by-step explanation:

To calculate the pressure inside the can, we need to calculate the mole fractions of each component and use Raoult's law. The mole fraction of ethyl alcohol (C2H5OH) can be calculated by dividing the moles of alcohol by the total moles of both alcohol and diethyl. The mole fraction of diethyl (C4H10) can be calculated similarly. Then, we can use Raoult's law, which states that the vapor pressure of a component in a mixture is equal to its mole fraction multiplied by its vapor pressure in the pure state. By multiplying the mole fraction of ethyl alcohol by its vapor pressure and adding it to the product of the mole fraction of diethyl and its vapor pressure, we can find the total pressure inside the can.

Let's calculate:

1. The moles of ethyl alcohol (C2H5OH):
2. 50 g / (46.1 g/mol) = 1.084 moles
3. The moles of diethyl (C4H10):
4. 40 g / (74.1 g/mol) = 0.539 moles
5. The mole fraction of ethyl alcohol:
6. 1.084 moles / (1.084 moles + 0.539 moles) = 0.668
7. The mole fraction of diethyl:
8. 0.539 moles / (1.084 moles + 0.539 moles) = 0.332
9. The pressure inside the can:
10. (0.668 x 0.08) + (0.332 x 0.7) = 0.114 + 0.232 = 0.346 atmospheres