t Experimental Determination of an Equilibrium Constant The decomposition of HI(
ID: 486070 • Letter: T
Question
t Experimental Determination of an Equilibrium Constant 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 Na2 S2 O3 (aq) The reaction of I2 with the titrant is Experimental data Data for the experiment are provided in this table nitial mass of HI Time Volume of titrant Bulb (hours) 0.300 20.96 2 0.320 4 27.90 32.31 0.315 12 0.406 41.50 20 28.68 0.280 40 Part AExplanation / Answer
Q=([H2]*[I2])/[HI]^2
Concentrations of H2= 5.378*10^-4 the concentation of I2=H2
Concentration of HI= 4.398*10^-3
Q=[Products]^coefficient/[Reactants]^cofficient=Kc
In this case the equation will be:
Q=Kc= [H2][I2]/[HI]^2
plugging values
Q=Kc=[5.378*10^-4][5.378*10^-4]/[4.398*10^-3]^2
Q=Kc= 1.5*10^-2 -------answer
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