One form of Raoult's Law states that the vapor pressure of a solution of a non-volatile solute at certain temperature is equal to the vapor pressure of the pure solvent at the same temperature multiplied by the mole fraction of the solvent, this is:
p = X solvent * P pure solvent,
X solvent = number of moles of solvent / total number of moles.
Here the solute is 13.6 g of C12 H10 and the solvent is 26.4 g C6H6.
=>
moles of solvent = mass in grams / molar mass
molar mass of C6H6 = 6 * 12 g/mol + 6 * 1g/mol = 78 g/mol
moles of solvent = 26.4 g / 78 g/mol = 0.33846 mol
molar mass of C12H10 = 12 * 12g/mol + 10*1g/mol = 154 g/mol
moles of solute = 13.6 g / 154 g/mol = 0.08831 mol
=> X solvent = 0.33846 / (0.33846 + 0.08831) = 0.793
=> p = 0.793 * 100.84 torr = 79.97 torr ≈ 80.0 torr
Answer: 80.0 torr
Answer:
Explanation: It has been given that the temperature of the water decreases when chromium chloride is dissolved in water. Thus fall in the temperature explains the fact that the bond energies of the reactants have more energy rather than the products.
a) Thus the heat of the solution is endothermic in nature as more energy is needed to break the reactant molecules.
b) The combined ionic bond strength of CrCl2 and inter molecular forces between water molecules must be stronger than the attractive forces between the water molecules and chromium and chloride ions as the reaction is endothermic in nature thus more energy would be required to break the bonds between the reactants hence making them more stronger.
Answer: The new volume be if you put it in your freezer is 1.8 L
Explanation:
To calculate the final temperature of the system, we use the equation given by Charles' Law. This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure.
Mathematically,

where,
are the initial volume and temperature of the gas.
are the final volume and temperature of the gas.
We are given:

Putting values in above equation, we get:

The new volume be if you put it in your freezer is 1.8 L
Answer:
Mass of hydrogen gas evolved is 0.0749 grams.
Explanation:
Total pressure of the gases = p = 758 mmHg
Vapor pressure of water = 23.78 mmHg
Pressure of hydrogen gas ,P = p - 23.78 mmHg = 758 mmHg - 23.78 mmHg
P = 734.22 mmHg = 
Temperature of of hydrogen gas ,T= 25°C =298.15 K
Volume of hydrogen gas = V = 0.949 L
Moles of hydrogen gas =n
PV = nRT (Ideal gas equation )

n = 0.03745 mol
Moles of hydrogen gas = 0.03745 mol
Mass of 0.03745 moles of hydrogen gas = 0.03745 mol × 2 g/mol = 0.0749 g
Mass of hydrogen gas evolved is 0.0749 grams.