In atmospheric chemistry, the following chemical reaction converts SO 2 , the pr

Question

In atmospheric chemistry, the following chemical reaction converts SO2, the predominant oxide of sulfur that comes from combustion of S-containing materials, to SO3, which can combine with H2O to make sulfuric acid (and thus contribute to acid rain): SO2(g) + 1/2 O2(g) -> SO3(l).

a) Write the expression for K for this equilibrium

b) Calculate the value of delta Go for this equilibrium using the deltafGo values in Appendix 2. (Appendix 2 values: SO2 = -300.13, O2 = 0, SO3 = -371.02)

c) Calculate the value of K for this equilibrium.

d) If 1.00 bar of SO2 and 1.00 bar of O2 are enclosed in a system in the presence of some SO3 liquid, in which direction would the reaction move?

Explanation / Answer

1)a

The equation for the K=[SO3]/[SO2][O2]1/22

1b) delta G0 = (heat of formation of products )-( f0 of reactants)

=(-371.02)-(-300.13+0)kj/mol

= -171.11kj/mol

1C) value of ln K= (-G0/RT)

logK = (171.11 ×1000)/(8.314×298×2.3)

R=gas constant= 8.314j/mol

Lnk = 2.303logk

T=298K

Logk=30

K = log10 + log 3

= 1.47

1d) Since the value of G0 >0 spontaneous

And K < 0 so reaction will favour the product

Hence reaction will be in forward direaction

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