The reactions, PCl₅ (g) $\stackrel{}{\rightleftharpoons }$ PCl₃(g) + Cl₂(g) and COCl₂(g) $\stackrel{}{\rightleftharpoons }$ CO(g) + Cl₂(g) are simultaneously in equilibrium in an equilibrium box at constant volume. A few moles of CO(g) are later introduced into the vessel. After some time, the new equilibrium concentration of

(1) PCl₅ will remain unchanged

(2) Cl₂ will be greater

(3) PCl₅ will become less

(4) PCl₅ will become greater

In the Haber process for the industrial manufacture of ammonia involving the reaction, N₂ + 3H₂ $\stackrel{}{\rightleftharpoons }$ 2NH₃ at 200 atm pressure in the presence of a catalyst, temperature of about 500°C. This is considered as optimum temperature for the process because

(1) yield is maximum at this temperature

(2) catalyst is active only at this temperature

(3) energy needed for the reaction is easily obtained at this temperature

(4) rate of the catalytic reaction is fast enough while the yield is also appreciable for this exothermic reaction at this temperature.

For the equilibrium of the reaction,\(\mathrm{HgO}(\mathrm{~s}) \rightleftharpoons \mathrm{Hg}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_ 2(\mathrm{~g}), \mathrm{K_P}\) for the reaction at a total pressure of "P" will be:

What is the minimum mass of CaCO3 (s), below which it decomposes completely, required to establish equilibrium in a 6.50 litre container for the reaction : [ K_C = 0.05 mole/litre]

CaCO₃ (s) $\stackrel{}{\rightleftharpoons }$ CaO(s) + CO₂(g)

(1) 32.5g

(2) 24.6 g

(3) 40.9g

(4) 8.0 gm

The value of k_p for the reaction at 27°C Br₂(l) + Cl₂(g) $\stackrel{}{\rightleftharpoons }$ 2BrCl(g) is '1 atom'. At equilibrium in a closed container partial pressure of BrCI gas is 0.1 atm and at this temperature the vapour pressure of Br₂(l) is also 0.1 atm. Then what will be minimum moles of Br₂(l) to be added to 1 mole of Cl₂ , initially, to get above equilibrium situation :

(1) $\frac{10}{6}$ moles

(2) $\frac{5}{6}$moles

(3) $\frac{15}{6}$moles

(4) 2 moles

5 mol PCI₅(g) and one mole N₂ gas is placed in a closed vessel. At equilibrium PCI₅(g) decomposes 20% and total pressure in to the container is found to be 1 atm. The k_P for equilibrium

PCl5(g) $\stackrel{}{\rightleftharpoons }$ PCl₃(g) + Cl₂(g)

(1) $\frac{1}{24}$atm

(2) $\frac{1}{4}$atm

(3) $\frac{1}{16}$atm

(4) $\frac{1}{28}$atm

The degree of dissociation of water in a 0.1 M aqueous solution of HCl at a certain temperature t°C is 3.6 x 10^–15. The temperature t must be :

(1) < 25°C

(2) = 25°C

(3) > 25°C

(4) insufficient data to predict

Which one is the correct expression below for the solution containing 'n' number of weak acids?

(1) ${\text{[H}}^{+}]=\sqrt{\sum _{i=1}^n\frac{K_i}{C_i}}$

(2) ${\text{[H}}^{+}]=\sqrt{\sum _{i=1}^n{K}_i{C}_i}$

(3) $\left[H^{+}\right]=\sum _{i\hspace{0.17em}=\hspace{0.17em}1}^n{K}_i{C}_i$

(4) none of these

The pH of glycine at the first half equivalence point is 2.34 and that at second half equivalence point is 9.60.At the equivalence point (The first inflection point) The pH is :

(1) 3.63

(2) 2.34

(3) 5.97

(4) 11.94

The pKa, of a weak acid if titration progress is monitored as follows

(1) Data insufficient

(2) 8.15

(3) 3.88

(4) 4.28