Useful universal constants:
R=8.314JK-1mol-1 = 8.205 × 10-2 atmK-1mol-1
C=3.0 × 108 m/s
NA=6.023 × 1023 mol-1
1 Torr=1.33 × 102 Nm-2
1 bar =1.0 × 105 NM-2
QUESTION ONE (30 MARKS).
A)Explain, with the examples where possible, the following:
i)work (2mrks)
ii)heat (2mrks)
iii)Bohr Temperture (2mrks)
iv)Order of a reaction(2mrks)
v)reaction mechanism (2mrks)
B)i)Explain why real gases deviate from ideal gas behavior (3mrks)
ii)State the principle of corresponding states.(1mrk)
iii)Estimate the critical constants of a gas with van der waals paremeters a= 0.751 atm L2mol-2 and b=0.0226 Lmol-1(3mrks)
C(i)Explain what is internal energy (U).
(ii) A mole of monoatomic gas at 1 bar and 273.15K is allowed to expand adiabatically against a constant pressure of 0.395 bar until equilibrium (CV =3/2 R)
a)Calculate the final volume.(2mrks)
b) Calculate the final temperature.(2mrks)
c)calculate the work done during the process.(2mrks).
D)(i) Consider the reaction
A + B ? products
From the following data at a given temperature determine the order and rate constant of the reaction: (4mrks)
(A)mol dm-3 (B)mol dm-3 rate(mol-1)
1.5 1.50 3.2 × 10-1
1.5 2.50 3.2 × 10-1
3.0 1.50 6.4 × 10-1
ii) The rate constant for the second order reaction:
2NO2(g) + 2NO(g) + O2(g) is 0.54Ms at 30oC
Calculate how long it will take for the concentration of NO2 to decrease from 0.62M to 0.28M (mrks)
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