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Conjugate acid of $SO_4^{2-}$ is

Which of the following is a Lewis acid ?

Which of the following are Lewis acids ?

For a reaction, $\ce{A <=> P}$, the plots of [A] and [P] with time at temperatures $T_1$ and $T_2$ are given below. If $T_2 > T_1$, the correct statement(s) is (are) (Assume $\Delta H^{\ominus}$ and $\Delta S^{\ominus}$ are independent of temperature and ratio of lnK at $T_1$ to lnK at $T_2$ is greater than $T_2 / T_1$ . Here $H, S, G$ and $K$ are enthalpy, entropy, Gibbs energy and equilibrium constant, respectively.)

What will be the expression of $ K_p $ for the given reaction if the total pressure inside the vessel is $ P $ and degree of dissociation of the reactant is $ a $ ? The reaction : $ \ce{N2O4 <=> 2NO2} $

An aqueous solution contains $0.10 \, M \, H_2S$ and $0.20 \, M \, HCl$ . If the equilibrium constants for the formation of $HS^-$ from $H_2S$ is $1.0 \times 10^{-7}$ and that of $S^{2- }$ from $HS^-$ ions is $ 1.2 \times 10^{-13}$ then the concentration of $S^{2-}$ ions in aqueous solution is -

A sample of $ HI_{(g)} $ is placed in a flask at a pressure of $ 0.2 $ atm. At equilibrium, partial pressure of $ HI_{(g)} $ is $ 0.04 $ atm. What is $ K_p $ for the given equilibrium ? $ \ce{2HI_{(g)} <=> H2_{(g)} +I2_{(g)}} $

What will be the equilibrium constant of the given reaction carried out in a $ 5 \,L $ vessel and having equilibrium amounts of $ A_2 $ and $ A $ as $ 0.5 $ mole and $ 2 \times 10^{-6} $ mole respectively ? The reaction : $ \ce{A2 <=> 2A} $

At a certain temperature in a 5 L vessel, 2 moles of carbon monoxide and 3 moles of chlorine were allowed to reach equilibrium according to the reaction,$CO + Cl_{2} <=> COCl_2 $ At equilibrium, if one mole of CO is present then equilibrium constant $(K_c)$ for the reaction is :