The equilibrium 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
Which one of the following information can be obtained on the basis of Le-Chatelier's principle ?
Dissociation constant of a weak acid
Entropy change in a reaction
Equilibrium constant of a chemical reaction
Shift in equilibrium position on changing values of a constant
K1 and K2 are equilibrium constant for reactions (i) and (ii)
Then,
K1 = (K2 )0
In the two gaseous reactions (i) and (ii) at 250o C.
the equilibrium constants K1 and K2 are related as
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
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
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
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
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
The rate of reaction depends upon the
volume
force
pressure
conc of reactants
