The decomposition of is represented by the equation 2HI <---> H2 + I2 The follow

Question

The decomposition of is represented by the equation

2HI <---> H2 + I2


The following experiment was devised to determine the equilibrium constant of the reaction.
HI is introduced into five identical 400-cm3 glass bulbs, and the five bulbs are maintained at 623 K.The amount of produced over time is measured by opening each bulb and titrating the contents with 0.0150 M . 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
() Time
() Volume of titrant
()
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
Part A
In which bulb would you expect the composition of gases to be closest to equilibrium?

I got bulb 5 for the correct answer but how to I calculate the KC value? for the decomp pf HI at 623K?

Explanation / Answer

bulb 5

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