Given the following two reactions:
     A + B ⇌ C + D, with rate constant K₁
     E + F ⇌ G + H, with rate constant K₂

If C + D + E + F produces a product, what is the rate constant for this reaction?

The equilibrium constant Kp for the following reaction is:

${{\mathrm{MgCO}}_3}_{\left(\mathrm{s}\right)}\rightleftharpoons {\mathrm{MgO}}_{\left(\mathrm{s}\right)}+{{\mathrm{CO}}_2}_{\left(\mathrm{g}\right)}$

1. $\mathrm{Kp<mspace\; width="1em"></mspace>}=\hspace{0.17em}{\mathrm{P}}_{{\mathrm{CO}}_2}$

2. $\mathrm{Kp}={\mathrm{P}}_{{\mathrm{CO}}_2}\times \frac{{\mathrm{P}}_{{\mathrm{CO}}_2}\times {\mathrm{P}}_{\mathrm{MgO}}}{{\mathrm{P}}_{{\mathrm{MgCO}}_3}}$

3. $\mathrm{Kp}=\frac{{\mathrm{P}}_{{\mathrm{CO}}_2}+{\mathrm{P}}_{\mathrm{MgO}}}{{\mathrm{P}}_{{\mathrm{MgCO}}_3}}$

4. $\mathrm{Kp}=\frac{{\mathrm{P}}_{{\mathrm{MgCO}}_3}}{{\mathrm{P}}_{{\mathrm{CO}}_2}\times {\mathrm{P}}_{\mathrm{MgO}}}$

For any reversible reaction, if we increase the concentration of the reactants, the 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 , ${\mathrm{BaO}}_2\left(\mathrm{s}\right)\rightleftharpoons \mathrm{BaO}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$; ∆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:

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$

is given by $\mathrm{Q}=\frac{{\left[{\mathrm{NH}}_3\right]}^2}{\left[{\mathrm{N}}_2\right]{\left[{\mathrm{H}}_2\right]}^3}$.
Under what conditions will the reaction proceed from right to left?

1. Q = K_C
2. Q < K_C
3. Q > K_C
4. Q = 0

(where K_C is the equilibrium constant)