then C + D + E + F ⇒ product. The constant of reaction will be:
1.
2.
3.
4. None of these
The equilibrium constant Kp for the following reaction is:
1.
2.
3.
4.
The correct relation between dissociation constants of a di-basic acid is:
1.
2.
3.
4.
For any reversible reaction, if we increase the concentration of the reactants, the effect on equilibrium constant will:
1. Depend on the amount of concentration
2. Remain unchanged
3. Decrease
4. Increase
The ionization constant of \(CH_{3} COOH\) is 1.7 × \(\left(10\right)^{- 5}\) and the concentration of \(H^{+ }\)ions is 3.4 × \(\left(10\right)^{- 4}\). The initial concentration of \(CH_{3} COOH\) will be:
1. 3.4 × \(\left(10\right)^{- 4}\)
2. 3.4× \(\left(10\right)^{- 3}\)
3. 6.8 × \(\left(10\right)^{- 4}\)
4. 6.8 × \(\left(10\right)^{- 3}\)
For a reaction , ; ∆H = + ve. At equilibrium condition, the pressure of O2 depends on the:
1. Increased mass of BaO2
2. Increased mass of BaO
3. Increased temperature on equilibrium.
4. Increased mass of BaO2 and BaO both.
The reaction quotient (Q) for the reaction:
is given by .
Under what conditions will the reaction proceed from right to left?
1. Q = KC
2. Q < KC
3. Q > KC
4. Q = 0
(where KC is the equilibrium constant)