In the two gaseous reactions (i) and (ii) are 250oC
the equilibrium constants K1 and K2 are related as
K2= 1/K1
K2= K11/2
K2= [1/K1]2
K2=K12
The equilibrium constant for the reaction A22A at 500k and 700k are 1x10-10 and 1x10-5. The given reaction is
exothermic
slow
endothermic
fast
Chemical reaction which proceeds in both forward and backward directions is called ____________
Substitution reaction
Double decomposition reaction
Irreversible reaction
Reversible reaction
For the reaction,
CH4(g) 2O2(g) CO2 (g) + 2H2O (l). ΔrH= 170.8 KJmol-1 which of the following statement 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 KP= [CO2] / [CH4][O2]
Addition of CH4 (g) or O2 (g) at equilibrium will cause a shift to the right.
The reaction is exothermic
The following equilibrium are given
N2+ 3H22NH3; k1
N2+ O2 2 NO; K2
H2+1/2 O2 H2O; K3
The equilibrium constant off the reaction 2NH3 +5/2O2 2NO+ 3H2O in terms of K1, K2 and K3 is
K1 K32 / 2
K2 K33/ k1
K1K2K3
K1K2/K3
The equilibrium constant of a reversible reaction at a given temperature _______________
Depends on initial concentration of the reactants
Depends on concentration of the products at equilibrium
Does not depend on the initial concentration
It is not a characteristic of the reaction
Reaction BaO2 (s) BaO(s) +O2 (g); ΔH= +ve. In equilibrium condition, pressure of O2 depends on
increased mass of BaO2
increased mass of BaO
Increased temperature of equilibrium
increased mass of BaO2 and BaO both
For a reversible reaction, if the concentration of the reactants are doubled, the equilibirum constant will be,
one -fourth
halved
doubled
the same
The rate of chemical reaction :
Increases the reaction proceeds
Decreases the reaction proceeds
May increase or decrease during the reaction
Remains constant as the reaction proceeds
For the equilibrium
Kp= PCO2
None of these
