The decomposition of HI(g) is represented by the equation 2HI(g)?H2(g)+I2(g) The

Question

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.

28.68

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

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

Explanation / Answer

The reaction most closest to the equilibrium will be reaction in bulb 5

It is being a trick question, no calculation is required as soon as you put some moles of HI, it will start to attain equilibrium by decomposing into H2 and I2. The more the time passes. the more rxn will become slower and will try to attain the equilibrium.

Hence bulb 5 will reach the equilibrium at the earliest

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