t Experimental Determination of an Equilibrium Constant The decomposition of HI(
ID: 940807 • Letter: T
Question
t Experimental Determination of an Equilibrium Constant The decomposition of HI(g) is represented by the equation 2HI(g)E 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 The amount of lo produced over time is measured by opening each bulb and titrating the contents with 0.0150 M Na2 S2 O3 (aq). The reaction of I2 with the titrant is I2 2Na S203 Na2S406 2Nal Experimental data Data for the experiment are provided in this table Initial mass of HI Time Volume of titrant Bulb Ours (mL 2 0.300 20.96 4 0.320 27.90 12 0.315 32.31 20 0.406 41.50 5 0.280 40 28.68 Part A n which bulb would you expect the composition of gases to be closest to equilibrium? bulb 1 bulb 2 bulb 3 bulb 4 bulb 5 Submit My Answers Give Up Correct You have enough information to calculate the value of Q at each time increment. However, the value of 2 after 40 hours (bulb 5) will be the best estimation of the equilibrium constant K of theExplanation / Answer
2HI(g) <===> H2(g) + I2(g)
let me take bulb one.
No of mole of HI = 0.3 / 127.91 = 0.00234 mol
concentration of HI = 0.00234/0.4 = 0.00585 M
at equilibrium
No of mole of I2 produced = (20.96/1000)*0.015*(1/2)
= 0.00016 mol
concentration of I2 = 0.00016/0.4 = 0.0004 M
concentration of H2 = 0.00016/0.4 = 0.0004 M
Kc = [H2][I2]/[HI]^2
= 0.0004^2 / (0.00585-2*0.0004)
= 3.168*10^(-5)
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