Use the data in part a (which were collect at 460°C and are equilibrium partial pressures) to determine K for the reaction: H2 (g) + I2 (g) <---> 2 HI (g), and complete the missing information for part b.
PH2 (atm) | PI2 (atm) | PHI (atm) | |
a | 6.47e-3 | 0.594e-3 | 0.0137 |
b | 3.84e-3 | 1.52e-3 | ? |
Is K and Kp the same value for the above reaction? Please show work.
(a). Sol :-
Equilibrium reaction is :
H2 (g) + I2 (g) <---------> 2 HI (g)
Pressure equilibrium constant (K) is the ratio of partial pressure of products to the partial pressure of reactants raise to power stoichiometric coefficient at equilibrium stage of the reaction.
K = PHI2 / PH2.PI2
K = (0.0137 atm)2 / (6.47 x 10-3 atm).(0.594 x 10-3 atm)
K = 48.837
-----------------------------
(b).
Again,
K = PHI2 / PH2.PI2
48.837 = PHI2 / (3.84 x 10-3 atm)(1.52 x 10-3 atm)
PHI = (48.837 x 3.84 x 10-3 atm x 1.52 x 10-3 atm)1/2
PHI = 1.69 x 10-2 atm
Hence, PHI = 1.69 x 10-2 atm
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