Consider the reaction A?B. The rate of reaction is 1.6 × 10-2 M/s when the concentration of A is 0.35M. Calculate the rate constant if the reaction is i)first order in A

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)
Question two
A)Explain three methods for determining the rate law.
B)The data for determining 2A ?A2? of a certain reaction in ethanol solution at 40oC is as follows:
(A)moldm-3 × 10-3 68 50.2 40.3 33.1 28.4 22.3 18.7 14.5
(t)/Min 0 40 80 120 160 240 300 420
Using half life method , determine the reaction order.
C) (i) Explain A and Ea factors in the Arrhenius equation.(2mrks)




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