sulfur dioxide in the effluent gases from coal -burning electric power plants is

Question

sulfur dioxide in the effluent gases from coal -burning electric power plants is one of the principal causes of acid rain. One method for reducing sol emissions involves partial reduction of soa to Hus, fonowed by the coewersion the Has and remaining soa to elemental sulfur: Substance 228.6 33.6 a) Predict whether the change in entropy for the reaction above would be positive or negative? Briefly explain. b) The value of AG" (in kl/mol) for sls) is c) Calculate the standard free energy (AG) using the data provided and your answer to part (b) d) is the reaction run under the conditions in part (c) spontaneous in the forward direction? Briefly explain. e) This reaction is exothermic. Using your answer in part high T low T all T (a), over what temperature range would you predict the forward reaction to be spontaneous (circle one) Briefly explain Calculate the equilibrium constant (K) for the reaction at 25 "C. g) Based on your answer in part (f), is the formation of products or reactants favored at 25 c? Briefly explain

Explanation / Answer

For the given reaction

a. we get 5 moles of gas from 3 moles of starting material, so the entropy is would be positive.

b. dG for S(s) is zero.

c. dGofrxn = (2 x -228.6) - (2 x -33.6 - 100.2)

                  = -289.8 kJ/mol

d. the reaction is spontaneous

e. Reaction being exothermic, it will be sponatneous over the temperature range of,

low T

f. equilibrium constant

dG = -RTlnK

-289800 = -8.314 x 298 lnK

K = 6.3 x 10^50

g. The formation of products is favoured over the reactants at 25 oC. K is very high and dG is -ve.

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