Problem 1.2: The equation below gives the boiling temperature of isopropanol as a function of pressure: B A-log10 P where Tis in kelvin, P is in bar, and the parameters A, B, and Care A = 4.57795, B = 1221.423, C=-87.474. T= C,

:) Using the ideal gas model, show that () (), ӘР ЭТ T V =-1

PHYSICAL CHEMISTRY:Calculate the pressure exerted by 1.0 mol C2H6 at 1000 K in 100 cm3 using (a) the ideal gas equation and (b) the van der Waals equation. The van der Waals constant for C2H6 are: a = 5.562 bar dm6 mol-2 ; b = 0.06380 dm3 mol-1 answer:[831; 1.72 x 10-3]

7.

For one of the substance ps in table 3.2 compute the change volume and work done by one kilogram of substance is heated from 15 C - 25 C at constant pressure of 1 bar

1. Calculate AU, AH, q, and w for the reversible isothermal expansion of 62.4 g of Ar from a volume of 2.50 L to 15.5 L at 150.0 K. a. Treat Ar as an ideal gas. b. Treat Ar as a gas with the equation of state given below where a represents the van der Waals attraction constant. (We are ignoring the constant b in this problem.) а (P+ -)V = RT V? m т c. Explain any difference between your answers to parts a and b.

Give a specific example of a system with the energy transformation shown. In the question, W is the work done on the system, and K, U, and Eth are the kinetic, potential, and thermal energies of the system, respectively. Any energy not mentioned in the transformation is assumed to remain constant; if work is not mentioned, it is assumed to be zero. W → ΔEth

This table displays the vapor pressure of nitrogen at several different temperatures. Use the data to determine the heat of vaporization and normal boiling point of nitrogen.Temperature (K)                        Pressure (torr)65                                              130.570                                              289.575                                              570.880                                              102885                                              1718