7.36 The normal melting point of Ni is 1452°C. The vapor pressure of liquid Ni is 0.100 torr at 1606°C and 1.00 torr at 1805°C. The molar heat of fusion of Ni is 4.25 kcal/mol. Making reasonable approximations, estimate the vapor pres- sure of solid Ni at 1200°C.

(3) Vapor pressure of liquid ethanol is 7291 Pa at 20°C. (a) one student reports that the vapor pressure is 31741 Pa at 52°C. Another student reports it to be 31741 Pa at 502°C. Which of the results is correct? Why? (b) calculate the normal boiling temperature of ethanol (assume Patm=101,325Pa).

(c) Is methane a solid, liquid, or gas at 1 atm and 0 °C? (d) If solid methane at 1 atm is heated while the pressure is held constant, will it melt or sublime? (e) If methane at 1 atm and 0 °C is compressed until a phase change occurs, in which state is the methane when the compression is complete?

7. (5)Consider the phase diagram given below atm ス50 T°C aら 50 15 100 |50 200 Identify the normal boiling point, and normal freezing point. fp. Which phase, solid or liquid is most densed? bp Indicate the Triple point and the critical point on the diagram.

The melting point of water at the pressure of the interest (1 atm) is 0 oC and the enthalpyof fusion is 6 kJmol-1. The boiling point is 100 oC and the enthalpy of vaporization is40kJmol-1.Calculate ΔH and ΔS for the transformation of 5 grams of H2O (ice) from (s, -10/X oC)to H2O (g, 1000/X oC)cp (water)= 75.3 joule/mole.K. cp (ice)=36.2 joule/mole.K x=4.5

The vapor pressure of the liquid HF is measured at different temperatures. The following vapor pressure data are obtained. Temperature, K P, mmHg 356.6 272.9 289.9 684.0 Calculate the enthalpy of vaporization (AHvap) in kJ/mol for this liquid. Submit kJ/mol Show Approach Hide Tutor Steps

Prior to the discovery that freon-12 (CF2C12) was harmful to the Earth's ozone layer, it was frequently used as the dispersing agent in spray cans for hair spray, etc. The enthalpy of vaporization at its normal boiling point of -29.2 °C is 20.25 kJ/mol. Assume AHvap to be independent of temperature and estimate the pressure of freon-12 in a can of hair spray at 40 °C.

Can you explain this problem? Where did the P1 came from? And can you redo the calculation?

Please don't provide hand writtin solution...

Suppose the vapor pressure of a substance is measured at twodifferent temperatures. (a) By using the Clausius–Clapeyronequation (Equation 11.1) derive the following relationshipbetween the vapor pressures, P1 and P2, and the absolute temperaturesat which they were measured, T1 and T2:   (b) Gasoline is a mixture of hydrocarbons, a componentof which is octane (CH3CH2CH2CH2CH2CH2CH2CH3). Octane has a vapor pressure of 13.95 torr at 25 °C and a vaporpressure of 144.78 torr at 75 °C. Use these data and the equationin part (a) to calculate the heat of vaporization of octane.(c) By using the equation in part (a) and the data given in part(b), calculate the normal boiling point of octane. Compareyour answer to the one you obtained from Exercise 11.81.(d) Calculate the vapor pressure of octane at -30 °C.