The following equilibria are given
The equilibrium constant of the reaction in terms of K1, K2 and K3 is
K1,K2,K3
If K1 and K2 are the respective equilbrium constants for the two reactions
The equilibrium constant of the reaction
will be
K1 / (K2 )2
K1 . K2
K1 / K2
K2 / K1
The equilbrium constants for the reaction at 500 K and 700 K are 1 × 10-10 and 1 × 10-5 . The given reaction is
exothermic
slow
endothermic
fast
The rate constants for forward and backward reaction of hydrolysis of ester are 1.1 × 10-2 and 1.5 × 10-3 per minute. Equilibrium constant for the reaction
CH3 COOC2H5+H+ CH3COOH + C2H5OH is
4.33
5.33
6.33
7.33
The dissociation constants for acetic acid and HCN at 25o C are 1.5 × 10-5 and 4.5 × 10-10 , respectively. The equilibrium constant for the equilibrium,
would be
3.0 × 103
3.0 × 10-5
3.0 × 104
3.33 × 104
K1 and K2 are equilinrium constant for reactions (i) and (ii)
Then,
K1 = (K2 )0
The value of equilibrium constant of the reaction
16
For the reaction,
Which of the following statements is not true ?
At equilibrium, the concentrations of CO2 (g) and H2O(l) are not equal.
The equilibrium constant for the reaction is given by
Addition of CH4 (g) or O2 (g) at equilibrium will cause a shift to the right
The reaction is exothermic
Reaction In equilibrium condition, pressure of O2 depends on
increased mass of BaO2
increased mass of BaO
increased temperature of equilbrium
increased mass of BaO2 and BaO both
For the equilibrium
which of the following expressions is correct ?
Kp = PCO2
