At 1 atm ,100 grams of benzene is vapourised to its boiling
point. Hvap=
94.4 cal/g
U=0= q+ W or,
q=-W We know that q=
Hvap=
94.4 cal/g
(a) W= -94.4 cal/g
(b) q= 94.4 cal/g
(c) Hvap=
94.4 cal/g
(d) U=0
?ideal concepts At 1 atm, 100 grams of benzene (CoHs) is vaporized at its boiling point...
The following information is given for benzene, CH at 1 atm: boiling point So.1 °C AHap(80.1 °C)=30.7 kJ/mol melting point AHfus(5.50 °C)9.95 kJ/mol 5.50 °C specific heat liquid 1.74 J/g°C At a pressure of 1 atm, what is AH in kJ for the process of condensing a 49.4 g sample of gaseous benzene at its normal boiling point of S0.1 °C kJ
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...
1. The normal (at 760 mmHg, or 1 atm) boiling point of water is 100°C. What mass of glucose (C6H202) would you have to dissolve in 1000 g of water to decrease the vapor pressure at 100°C by 1%? Assume that water follows Raoult's law. M(H2O) = 18.02 g/mol, M(C6H1206) = 180.2 g/mol. (10 pts) 2. What is the normal boiling point of such a solution? Assume ideal behavior. The ebullioscopic (boiling-point elevation) constant of water is Kp = 0.512...
The boiling temperature of nitrogen at atmospheric pressure at sea level (1 atm pressure) is -196°C. Therefore, nitrogen is commonly used in low-temperature scientific studies since the temperature of liquid nitrogen in a tank open to the atmosphere will remain constant at -196°C until it is depleted. Any heat transfer to the tank will result in the evaporation of some liquid nitrogen, which has a heat of vaporization of 198 kJ/kg and a density of 810 kg/m3 at 1 atm....
P2) (50 pts.) The boiling temperature of nitrogen at atmospheric pressure at sea level (1 atm pressure) is -196°C. Therefore, nitrogen is commonly used in low-temperature scientific studies, since the temperature of liquid nitrogen in a tank open to the atmosphere will remain constant at -196°C until it is depleted. Any heat transfer to the tank will result in the evaporation of some liquid nitrogen, which has a heat of vaporization of 198 kJ/kg and a density of 810 kg/m3...