For the reaction \(A\left(g\right) \rightleftharpoons 2B\left(g\right)\), the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500, at 1000 K.
[Given : R = 0.0831 L atm mol^-1 K^-1]K_p for the reaction at 1000 K is

Conjugate base for Bronsted acids H₂O and HF are

The major product of the following reaction is

MY and NY₃, two nearly insoluble salts have the same K_sp values of 6.2 × 10^-13 at room temperature. Which statement would be true in regard to MY and NY₃ ?

Phosphoric acid ionizes in three steps with their ionization constant values
\(Ka_1\), \(Ka_2\), and \(Ka_3\), respectively,while K is the overall ionization constant.
Which of the following statements are true?
A. \(\text{log} K\) = \(\text{log} Ka_1\) + \(\text{log}Ka_2\) +\(\text{log}Ka_3\)

B. \(H_3PO_4\) is a stronger acid than \(H_2PO_4^-\) and \(HPO_4^{2-}\).

С. \(Ka_1\) > \(Ka_2\) > \(Ka_3\).

D. \(\displaystyle Ka_1\,= \,\frac{Ka_3\,+\,Ka_2}{2}\).
Choose the correct answer from the options given below:

Higher yield of NO in
\(N_2\left(8\right)\, +\, O_2\left(g\right)\, \rightleftharpoons\, 2NO\left(g\right)\) can be obtained at
[\(\Delta H\) of the reaction = +180.7 kJ mol^-1]
A. higher temperature
B. lower temperature
C. higher concentration of N₂
D. higher concentration of O₂
Choose the correct answer from the options given below:

For the reaction \(2A \rightleftharpoons B + C, \, K_c \, = \, 4 \times 10^{-3}\). At a given time, the composition of reaction mixture is:
\([A]\, =\, [B]\, = \, [C]\, =\, 2 \times 10^{-3}\,M\)
Then, which of the following is correct?

In which of the following equilibria, \(\text{K}_\text{P}\) and \(\text{K}_\text{C}\) are NOT equal?

Consider the following reaction in a sealed vessel at equilibrium with concentrations of
\(\text{N}_2\,=\,3.0 \times 10^{-3}\text{M}\),
\(\text{O}_2\,=\,4.2 \times 10^{-3}\text{M}\),
\(\text{NO}\,=\,2.8 \times 10^{-3}\text{M}\),
\(2\text{NO}\left(g\right)\,\rightleftharpoons\, \text{N}_2\left(g\right)\,+\, \text{O}_2\left(g\right)\),
If \( 0.1\text{molL}^{-1}\) of \(\text{NO}\left(g\right)\) is taken in a closed vessel, what will be degree of dissociation \(\left(\alpha\right)\) of \(\text{NO}\left(g\right)\) at equilibrium?

Amonst the given options which of the following molecules/ion acts as a Lewis acid?

The equilibrium concentrations of the species in the reaction \(A\,+\,B\, \rightleftharpoons\, C \,+\,D\) are 2, 3, 10, and 6 mol L^-1, respectively at 300 K. \(\delta G^\circ\) for the reaction is (R = 2 cal/mol K).

The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is
[Given aK_a, of CH₃COOH = 4.57]

What mass of 95% pure CaCO₃ will be required to neutralise 50 mL of 0.5 M HCl solution according to the following reaction?

[Calculate upto second place of decimal point]

\(\text{3O}_2\,\left(g\right) \rightarrow\, \text{2O}_3 \left(g\right) \)
for the above reaction at 298 K, K_c is found to be \(3.0 \times 10^-{59}\). If the concentration of O₂ at equilibrium is 0.040 M then concentration of O₂ in M is

The pK_b of dimethylamine and pk_a of acetic acid are 3.27 and 4.77 respectively at T (K). The correct option for the pH of dimethylammonium acetate solution is:

Which will make basic buffer ?

The compound that is most difficult to protonate is

For the chemical reaction
N₂(g) + 3H₂(g) \(\rightleftharpoons\) 2NH₃(g)
the correct option is

pH of a saturated solution of Ca(OH)₂ is 9. The solubility product (k_sp) of Ca(OH)₂ is

Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations:
A. \( \text{60 mL} \frac{\text{M}}{\text{10}}\)HCl + \( \text{40 mL} \frac{\text{M}}{\text{10}}\)NaOH
B. \( \text{55 mL} \frac{\text{M}}{\text{10}}\)HCl + \( \text{45 mL} \frac{\text{M}}{\text{10}}\)NaOH
C. A. \( \text{75 mL} \frac{\text{M}}{\text{5}}\)HCl + \( \text{25 mL} \frac{\text{M}}{\text{5}}\)NaOH
D. \( \text{100 mL} \frac{\text{M}}{\text{10}}\)HCl + \( \text{100 mL} \frac{\text{M}}{\text{10}}\)NaOH
pH of which one of them will be equal to 1 ?

The solubility of BaSO₄ in water is 2.42 × 10^–3gL^–1 at 298 K. The value of its solubility product (K_sp) will be
(Given molar mass of BaSO4 = 233 g mol–1)

Which one of the following conditions will favour maximum formation of the product in the reaction,
A₂(g) + B₂(g) \(\rightleftharpoons \) X₂(g) \(\Delta_r\)H = -XkJ?

The equilibrium constants of the following are:
N₂ + 3H₂ \(\rightleftharpoons\) 2NH₃ ------ K₁
N₂ + O₂ \(\rightleftharpoons\) 2NO ------ K₂
H₂ + \(\frac{\text{1}}{\text{2}}\)O₂ \(\rightarrow \) H₂O ------ K₃
The equilibrium constant (K) of the reaction:
2NH₃ + \(\frac{\text{5}}{\text{2}}\)O₂ \(\rightleftharpoons\) 2NO + 3H₂O, will be

Concentration of the Ag+ ions in a saturated solution of Ag₂C₂O₄ is 2.2 × 10^–4mol L^–1. Solubility product of Ag₂C₂O₄ is

A 20 litre container at of 400 K contains CO₂(g) at pressure 0.4 atm and an excess SrO (neglect the volume of solid SrO). The volume of the containers is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when pressure of CO₂ attains its maximum value, will be
[Given : SrCO₃(s) \(\rightleftharpoons\) SrO(s) + CO₂ (g).
K = 1.6 atm]

The product obtained as a result of a reaction of nitrogen with CaC₂ is

Among the following , the correct order of acidity is

Which of the following statements is false ?