Sol. In case of ideal solution the heat of solution is equal to the heat of the fusion solid component and activity of the solution becomes equal the mole fraction .
So the formula will be modified to:
; where
= mole
fraction
t = Temperature of the solution
= melting point of the
solute
= enthalpy of fusion
R = Universal constant
Since the ideal solution, so the mole fraction is equal to the solubility of the solute in the solution since in case of ideal solution we assume dilute solutions to be there.
Calculate the solubility of p-dibromobenzene in benzene at 20°C and 40°C assuming ideal solutions are formed....
4. Assuming ideal solution conditions, calculate the solubility of p-dibromobenzene in benzene at (a) 15°C and (b) 30°C. The standard melting point of p-dibromobenzene is 87.0°C and its enthalpy of fusion is equal to 13.2 kJ/mol. (8 pts)
The melting points and heats of fusion of o-, p-dinitrobenzene
are 390.1 and 446.7K, and 16.33 and 14.00 kJ/mol, respectively.
Assuming ideal solubility behavior, calculate the melting point for
a solution of 10 mol% o-dinitrobenzene in 90 mol%
p-dinitrobenzene.
6. The melting points and heats of fusion of o-, p-dinitrobenzene are 390.1 and 446.7 K, and 16.33 and 14.00 kJ/mol, respectively. Assuming ideal solubility behavior, calculate the melting point for a solution of 10 mol% o-dinitrobenzene in 90 mol% p-...
The enthalpy of fusion for benzene (C6H6, 78.0 g/mol) is 127.40 kJ/kg, and its melting point is 5.5°C. What is the entropy change when 1 mole of benzene melts at 5.5°C?
calculate the heat required to melt 9.73 g of benzene
at it's normal melting point
nd Phases (References] a. Calculate the heat required to melt 9.73 g of benzene at its normal melting point. Heat of fusion (benzene) 9.92 kJ/mol Heat = kJ b. Calculate the heat required to vaporize 9.73 g of benzene at its normal boiling point. Heat of vaporization (benzene) = 30.7 kJ/mol Heat = kJ Submit Answer Try Another Version 2 item attempts remaining arch о...
Benzene and toluene form nearly ideal solutions. The boiling point of pure benzene is 80.1°C. Calculate the chemical potential of benzene relative to that of pure benzene when χbenzene = 0.30 at its boiling point. If the activity coefficient of benzene in this solution were actually 0.93 rather than 1.00, what would be its vapor pressure?
1) Benzene and toluene form nearly ideal solutions. At 20°C the vapor pressure of pure benzene is 74 torr and that of pure toluene is 22 torr. A solution consisting of 1.00 mol of each component is boiled by reducing the external pressure below the vapor pressure. Calculate (a) the pressure at which boiling begins and (b) the composition of each component in the vapor.
1. The normal boiling point of benzene (i.e., at 1 atm) is 80.09 °C. The molar enthalpy of vaporization is 30.72 kJ mol . Assuming that AvapHm and AvapSm stay constant at their values at 80.09°C, calculate the values of AvapGm at 75.0 °C, 80.09 °C and 85.0 °C. Given your calculated values, do you still expect benzene to spontaneously condense at 75.0 °C and to spontaneously evaporate at 85.0°C? -1 2. The vapor pressure of a liquid was measured...
6. Benzene and toluene form nearly ideal solutions. The boiling point of pure benzene is 80.1°C. Calculate the chemical potential of benzene relative to that of pure benzene when Xbenzene = 0.30 at its boiling point. If the activity coefficient of benzene in this solution were actually 0.93 rather than 1.00, what would be its vapor pressure?
For benzene, C6H6, the heat of fusion at its normal melting point of 6 °C is 10.0 kJ/mol. The entropy change when 1.86 moles of liquid C6H6 freezes at 6 °C, 1 atm is ? J/K.
Q4. (3 marks) Estimate the freezing point of 150 cm of water to which 13.0 g of sucrose (molar mass = 342.29 g/mol) has been added. Kf of water is 1.86 K kg mol-? Q5. (5 marks) The ideal solubility of solute B at temperature T is given by AfusH1 In Xg RT Where Arush is the enthalpy of fusion of solute and Te is the freezing point of solute. Estimate the ideal solubility of lead in bismuth (as kg...