Question

1. In meteorology, pressures are expressed in units of millibars (mbar). Convert 1085 mbar to torr, Pascals, and to atmospheres. 2. Research in surface science is carried out using high vacuum (< 10-8 torr) or ultrahigh vacuum (<10-9 torr) chambers to reduce the surface contamination. How many molecules are there in a 1.00 cm3 volume inside such an apparatus at 298 K with pressure of 10-11 torr? What is the corresponding molar volume at this pressure and temperature? 3. Use the van der Waals equation and the Redlich-Kwong equation to calculate the value of the pressure of one mole of propane at 400 K confined to a volume of 100 cm3 . The experimental value is 333 atm. 4. Use the data below for CH4 (g) at 275 K to determine B2V at 275 K. P/bar 0.05 0.15 0.25 0.35 0.50 0.65 0.80 (Z-1)/10-4 0.7582 2.2613 3.7500 5.2730 7.5260 9.7781 12.0000 5. Using the Lennard-Jones parameters given in Table 2.7, estimate the covalent bond strength and distance for an O2 molecule. To calculate the depth of a typical L-J potential from the information in the table, you will need to realize that the Boltzmann constant has units of per particle (not per mole). 6. Use Equation C.9 in your textbook to derive the Maclaurin series of the following functions: (a) ln(1+ x), and (b) sin x

Answer 1

Part 1.) We know that, 1mbar=100pa.

So 1085mbar=1085×100pa=1.085×10⁵ answer.

And, 1mbar=0.7500637torr.

So 1085mbar = 1085×0.7500637torr=813.82torr answer

And, 1mbar=9.87×10^-4ATM

So 1085mbar=1085×9.87×10^-4=1.070811atm answer.

Part 2.) By PV=nRT

n=PV/RT=0.013atm×0.01litre/(0.082057×298K)

n=5.316×10^-6moles answer.

And molar volume=moles × volume=0.01×5.316×10^-6

So, molar volume= 5.316×10^(-8) mole-litre answer.

Part 3.) By vander wall equation-

(P+a/v²)(v-b)=RT

P=(RT/(v-b))-(a/v²)

-we have R=0.082057, T=400K, V=1litre, a=8.779, b=0.08445.

So, P=270.7332atm