Match the following: Column I Column II A. Gas constant (R) (p) mol dm^-3 B. Ionic product of wa

step 1 Dear students, in the given problem, problem 191 of chapter 2nd, you have asked to match the fol

Match the following: Column I Column II A. Gas constant (R)...

Match the following: Column I Column II A. Gas constant (R) (p) $\mathrm{mol} \mathrm{dm}^{-3}$ B. Ionic product of water (q) $\mathrm{mol}^{2} \mathrm{dm}^{-6}$ $(\mathrm{Kw})$ C. Van der Waal's con- (r) $\mathrm{dm}^{3}$ atm $\mathrm{K}^{-1} \mathrm{~mol}^{-1}$ stant (A) D. Equilibrium constant (s) $\mathrm{dm}^{6}$ atm $\mathrm{mol}^{-2}$ of $\mathrm{HA}_{c}(\mathrm{k})$

Match the following:
Column I Column II
A. Gas constant (R)
(p) $\mathrm{mol} \mathrm{dm}^{-3}$
B. Ionic product of water
(q) $\mathrm{mol}^{2} \mathrm{dm}^{-6}$
$(\mathrm{Kw})$
C. Van der Waal's con-
(r) $\mathrm{dm}^{3}$ atm $\mathrm{K}^{-1} \mathrm{~mol}^{-1}$
stant (A)
D. Equilibrium constant
(s) $\mathrm{dm}^{6}$ atm $\mathrm{mol}^{-2}$
of $\mathrm{HA}_{c}(\mathrm{k})$

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Key Concepts

Equilibrium Constant

The equilibrium constant quantifies the ratio of the concentration or pressure of products to reactants in a reversible chemical reaction at equilibrium. It serves as a measure of the position of equilibrium and is crucial in predicting the extent of reactions.

Gas Constant

The gas constant is a proportionality factor in the ideal gas law that relates the energy scale to the temperature scale. It bridges the macroscopic and microscopic properties of gases in equations, such as PV = nRT, and its value depends on the system of units used.

Ionic Product of Water

The ionic product of water is a measure of the extent of water’s autoionization into hydronium and hydroxide ions. It quantifies the equilibrium reached between these ions in pure water and is fundamental in understanding pH and acid-base balance.

Van der Waals Constant

Van der Waals constants are parameters in the van der Waals equation, which adjusts the ideal gas law to account for the finite size of molecules and intermolecular forces. These constants allow for more accurate predictions of real gas behavior compared to the ideal gas model.

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