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
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
If K1 and K2 are the respective equilibrium constants for the two reactions
The equilibrium constant of the reaction
will be
K1 / (K2 )2
K1 . K2
K1 / K2
K2 / K1
According to Le-Chatlier's principle, adding heat to a solid liquid equilibrium will cause the
temperature to increase
temperature to decrease
amount of liquid to decrease
amount of solid to decrease
For a reversible reaction, if the concentration of the reactants are doubled, the equilibrium constant will be
one-fourth
halved
doubled
the same
The value of equilibrium constant of the reaction
16
If the concentration of OH- ions in the reaction is decreased by times, then equilibrium concentration of Fe3+ will increase by
8 times
16 times
64 times
4 times
If is the fraction of HI dissociated at equilibrium in the reaction, starting with the 2 moles of HI, then the total number of moles of reactants and products at equilibrium are
K1 and K2 are equilibrium constant for reactions (i) and (ii)
Then,
K1 = (K2 )0
The rate of reaction depends upon the
volume
force
pressure
conc of reactants
