The reaction quotient (Q) for the reaction
The reaction will proceed towards right side if
Q > Kc
Q = 0
Q = Kc
Qc
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
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 equilibrium constant will be,
one -fourth
halved
doubled
the same
The rate constants for forward and backward reactions of hydrolysis of ester are 1.1 x 10-2 and 1.5 x 10-3 per minute. Then the equilibrium constant for the reaction is CH3COOC2H5 + H+ CH3COOH + C2H5OH is
4.33
5.33
6.33
7.33
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
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 value of a constraint
The rate of reaction depends upon the
volume
force
pressure
concentration of reactants
In an exothermic reaction, with the rise of temperature, the equilibrium constant
Decreases
Increases
Remains unchanged
None of these
