When 0.0430 mol of HI is heated to 500 K in a 5.00 L sealed container, the resulting equilibrium mixture contains 2.85 g of HI. Calculate Kc and Kp for the following decomposition reaction. 2 HI (g) H2 (g) + I2 (g)
2 HI (g) H2 (g) + I2 (g).
Kc = [HI]2 HI moles = 0.0430, the volume = 5L
HI concentration (Molarity) = Moles/ litre
Kc = [0.0086]2
Kc = 7.396 x 10-5.
Kp = Kc[RT]n R = Ideal gass constant = 8.314 jk-1mol-1.
n = Gaseous product mole no - gaseous reactant mol no.
n = 2-2
n = 0
Kp = Kc[RT]n T = 500 K (according to the question).
Kp = 7.396 x 10-5[8.314x500]0
Kp = 7.396 x 10-5.
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