The decomposition of hi(g) is represented by the equation
2hi(g) = h2(g) + i2(g)
the following experiment was devised to determine the equilibrium constant of the reaction.
hi (g) is introduced into five identical 400-cm3 glass bulbs, and the five bulbs are maintained at 623 k. the amount of i2 produced over time is measured by opening each bulb and titrating the contents with 0.0150 m na2s2o3 (aq). the reaction of i2 with the titrant is
i2 + 2na2s2o3 = na2s4o6 + 2nai
data for the experiment are provided in this table.
bulb initial mass of hi (g) time(hours) volume of titrant(ml)
1 0.300 2 20.96
2 0.320 4 27.90
3 0.315 12 32.31
4 0.406 20 41.50
5 0.280 40 28.68
what is the value of kc for the decomposition of hi at 623 k?

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