# Problem: The decomposition of HI(g) is represented by the equation2HI(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 isI2 + 2Na2S2O3 = Na2S4O6 + 2NaIData 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 28.68In which bulb would you expect the composition of gases to be closest to equilibrium?

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Chemical equilibrium: no net change in the concentration of reactants and products ###### Problem Details

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

In which bulb would you expect the composition of gases to be closest to equilibrium?