Determine the Kc for the following reaction at 355 K if 4.00 moles each of I2 and Cl2 were entered initially into an empty 5.00 liter flask. At equilibrium, 1.09 moles of ICl were measured (at 355K). 2 ICl (g) <-> I2 (g) + Cl2 (g) a) 0.189 b) 10.0 c) 7.43 d) 6.56 e) 0.846 f) 0.0543
Determine the Kc for the following reaction at 355 K if 4.00 moles each of I2 and Cl2 were entered initially into an empty 5.00 liter flask. At equilibrium, 1.09 moles of ICl were measured (at 355K). 2 ICl (g) <-> I2 (g) + Cl2 (g)
a) 0.189 b) 10.0 c) 7.43 d) 6.56 e) 0.846 f) 0.0543
Given , moles of I2 initially = 4.00 mol
moles of Cl2 initially = 4.00 mol
volume of flask = 5.00 L
moles of ICl at equilibrium = 1.09 mol
Now, let us calculate the concentration of each species,
Initial concentration of I2 = Moles of I2 initially/Volume
= 4.00 mol/5.00L
= 0.8 M
Initial concentration of Cl2 = Moles of Cl2 initially/Volume
= 4.00 mol/5.00L
= 0.8 M
Equilibrium concentration of ICl = Moles of ICl at equilibrium/Volume
= 1.09 mol/5.00L
= 0.218 M
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