At 1127 K and 1 atm pressure, a gaseous mixture of CO and CO₂ in equilibrium with solid carbon has 90.55% CO by mass. 

${\mathrm{C}}_{\left(\mathrm{s}\right)}$ $+$ ${{\mathrm{CO}}_2}_{\left(\mathrm{g}\right)}$ $\rightleftharpoons 2{\mathrm{CO}}_{\left(\mathrm{g}\right)}$

At the specified temperature, K_c for this reaction would be

$1.$ $0.25$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$
$2.$ $0.34$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$
$3.$ $0.15$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$
$4.$ $1.25$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$

1. Only reaction (a)
2. Both reactions (a) and (b)  
3. Only reaction (c)
4. Only reaction (b) 

For the reaction, $3{\mathrm{O}}_2$ $\left(\mathrm{g}\right)$ $\rightleftharpoons$ $2{\mathrm{O}}_3$ $\left(\mathrm{g}\right),$ ${\mathrm{K}}_{\mathrm{c}}$ $=$ $2.0$ $\times$ ${10}^{-50}$ L/mol at 25^°C. If the equilibrium concentration of O₂ in air at 25^°C is $1.6$ $\times$ ${10}^{-2}$, the concentration of O₃ would be: 

$1.$ $2.86$ $\times {10}^{28}$ $\mathrm{M}$
$2.$ $28.66$ $\times$ ${10}^{-28}$ $\mathrm{M}$
$3.$ $1.43$ $\times$ ${10}^{-28}$ $\mathrm{M}$
$4.$ $2.86$ $\times$ ${10}^{-28}$ $\mathrm{M}$

Consider the following reaction:

${\mathrm{CO}}_{\left(\mathrm{g}\right)}$ $+$ $3{{\mathrm{H}}_2}_{\left(\mathrm{g}\right)}$ $\rightleftharpoons$ ${{\mathrm{CH}}_4}_{\left(\mathrm{g}\right)}$ $$ $+$ ${\mathrm{H}}_2{\mathrm{O}}_{\left(\mathrm{g}\right)}$ $$

If the reaction mixture contains 0.30 mol of CO, 0.10 mol of H_2, and 0.02 mol of H₂O, and an unknown amount of CH₄ at equilibrium at 1300 K in a 1L flask, the concentration of CH₄ in the mixture will be -

(K_c = 3.90 at 1300 K) 

$1.$ $5.85$ $\times$ ${10}^2$ $\mathrm{M}$
$2.$ $5.85$ $\times$ ${10}^{-1}$ $\mathrm{M}$
$3.$ $5.85$ $\times$ ${10}^3$ $\mathrm{M}$
$4.$ $5.85$ $\times$ ${10}^{-2}$ $\mathrm{M}$

The concentration of hydrogen ion in a sample of soft drink is $3.8$ $\times {10}^{-3}$ $\mathrm{M}$. The  pH of the soft drink will be:

1. 3.14

2. 2.42

3. 11.58

4. 6.00

The pH of a sample of vinegar is 3.76. The concentration of H⁺ ions in the sample will be -

$1.$ $1.74$ $\times$ ${10}^{-4}$ $\mathrm{M}$
$2.$ $2.34$ $\times$ ${10}^{-11}\mathrm{M}$
$3.$ $2.86$ $\times$ ${10}^{-10}$ $\mathrm{M}$
$4.$ $1.74$ $\times$ ${10}^{-3}$ $\mathrm{M}$

The pH value of a 0.01 M solution of an organic acid is 4.15. The pK_a of the acid will be:

$1.$ $8.95$
$2.$ $1.43$
$3.$ $3.56$
$4.$ $6.30$

A solution containing 2 g of TlOH in 2 litres of water has a pH of?

(Atomic wt of Tl =204)

When 1mL of 13.6 M HCl is diluted with water to give 1 litre of solution, the pH of the resultant solution will be:

A 0.001 M aniline solution has a pH of:
(\(K_b = 4.27 \times 10^{-10}\))