Chemical EquilibriumHard
Question
Consider the following equilibrium in a closed container N2O4(g) ⇋ 2NO2(g) At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statements hold teue regarding the equilibrium constant (Kp) and degree of dissociation (α) ?
Options
A.Neither Kp nor α changes
B.Both Kp and α changes
C.Kp changes but α does not change
D.Kp does not change but α changes
Solution
For the reaction; N2O4(g) ⇋ 2NO2(g)
KC =
........(1)
where a is initial mole of N2O4 in V litre vessel and α is degree of dissociation of N2O4. If volume is reduced to V/2 , the initial concentration of N2O4 becomes
An increase in concentration of reactants leads to foward reaction i. e., the decomposition of N2O4 to have constant value of Kp.
KC =
........(1)where a is initial mole of N2O4 in V litre vessel and α is degree of dissociation of N2O4. If volume is reduced to V/2 , the initial concentration of N2O4 becomes
An increase in concentration of reactants leads to foward reaction i. e., the decomposition of N2O4 to have constant value of Kp.
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