List of practice Questions

Which of the following is the correct order of bond length?

Given below are two statements.
Statement I: HX bond length is higher in HCl than HF.
Statement II: The lowest boiling point in hydride of group 15 element is having covalency 4.

Find the formal charge of $ O $, $ O $, $ O $, and $ N $ respectively.

Out of the following, how many compounds have tetrahedral geometry?
\text{NH}_4^+, \, \text{XeF}_4, \, [\text{NiCl}_4]^{2-}, \, [\text{PtCl}_4]^{2-}, \, [\text{Cu(NH}_3\text{)}_4]^{2+}, \, \text{BF}_3, \, [\text{Ni(CO)}_4]

For $\text{XeO}_2\text{F}_2$, select the correct statements : (A) It has see-saw shape (B) $\angle FXeF \approx 180^\circ$ (C) $\angle OXeO \approx 180^\circ$ (D) Number of valence electron on $\text{Xe} = 5$

Select correct statements(s) (A) $\text{NF}_3$ has more dipole moment than $\text{NH}_3$ (B) $\text{O}_2^{2-}$ and $\text{F}_2$ both have same bond order (C) In $\text{O}_3$ central oxygen atom has $+1$ formal charge (D) In $\text{NO}_2$ all the atoms follow octet rule, so it is stable. (E) $\text{BeH}_2$ is planar

Statement-I : Among $\text{BF}_4^-$, $\text{SiF}_4$, $\text{SF}_4$, and $\text{XeF}_4$, the bond lengths are not identical in two of these molecules.
Statement-II : Among $\text{O}_2^+$, $\text{O}_2$, $\text{O}_2^{2-}$ and $\text{F}_2$ the highest bond order is found in $\text{O}_2^-$.

Match isostructural species in Column I with Column II.

Statement-I : The boiling point order is $ \mathrm{HF>HI>HBr>HCl} $
[2mm] Statement-II : The melting point order is : $ \mathrm{HI>HF>HBr>HCl} $

Given below are two statements: Statement–I: $K_H$ is constant with change in concentration of gas till the solution is dilute at a given temperature. Statement–II: According to Henry’s law, the partial pressure of gas in vapour phase is inversely proportional to the mole fraction of gas in solution.

Statement-I: K$_h$ for ideal dilute solution does not change with varying the concentration of solute.
Statement-II: K$_h$ for solution having same gas solute is independent of nature of solvent?

In the reaction sequence shown below, what is the mass (in grams) of product (C) formed?

10 mL of $2\,\text{M}$ NaOH solution is added to 20 mL of $1\,\text{M}$ HCl solution kept in a beaker. Now, 10 mL of this mixture is poured into a volumetric flask of 100 mL containing 2 moles of HCl and the volume is made up to the mark with distilled water. The solution in this flask is:

Osmotic pressure of a solution is 12 atm. What is the concentration of NaCl solution which is isotonic to the given solution at 900 K? Given $ R = 0.082 \, \text{L-atm K}^{-1} \text{mol}^{-1} $ (Assume 100% dissociation)

5 g of a solute X (M. wt = 200 g/mol) is dissolved in 250 g benzene. If $ \Delta T_f = 0.5 \, \text{K} $ and the relative lowering of vapour pressure is $ P \times 10^4 $, find $ P $. Given: $ K_f = 5.5 \, \text{K} \, \text{kg} \, \text{mol}^{-1} $, solute dimerises in benzene.

Given below are two statements:
Statement-I: $ K_H $ is constant with change in concentration of gas till solution is dilute at a given temperature.
Statement-II: According to Henry’s Law, partial pressure of gas in vapor phase is inversely proportional to mole fraction of gas in solution.

Choose the correct graph for the mixture of the volatile liquid CS$_2$ and acetone.

Two solutes, $0.3 \text{ gm}$ of $\text{A}$ ($M_w = 60 \text{ gm/mol}$) & $0.9 \text{ gm}$ of $\text{B}$ ($M_w = 180 \text{ gm/mol}$) are dissolved in $100 \text{ ml}$ solution. Find osmotic pressure of solution at $300 \text{ K}$ (in $\text{atm}$) ($\text{R} = 0.082 \text{ atm}-\text{L/mol-K}$)

Salt ($\text{X}$) is soluble in water. Salt ($\text{Y}$) is sparingly soluble in water. Salt ($\text{Z}$) is soluble only in hot water. $\text{X}, \text{Y}, \text{Z}$ respectively are.

If pure liquids A and B have vapour pressures of 55 kPa and 15 kPa respectively. If in a solution of A and B, mole fraction of A in vapour is 0.8, then find mole fraction of A in liquid phase.

If percentage of N$_2$ above a liquid solution is 80% at a total pressure of 10 atm, then find the mole fraction of N$_2$ gas dissolved in solution.
[Given that Henry’s constant for N$_2$ is $7.6 \times 10^7$ mm Hg]

2 moles of liquid A and 3 moles of liquid B are mixed to from an ideal solution. The vapour pressure of ideal solution is 320 mm Hg. When 1 mole of A & 1 mole of B is further added then new vapour pressure of solution is 328.57 mm Hg. Find the vapour pressure of pure A ($P_A^\circ$) & pure B ($P_B^\circ$):

Arrange the given metal ions in increasing order of number of unpaired electrons in the low spin complexes formed by $ \text{Mn}^{3+}, \text{Cr}^{3+}, \text{Fe}^{3+}, \text{Co}^{3+} $

An element ‘M’ does not evolve H$_2$ gas on treatment with dilute HCl. MSO$_4$ (1 mol) on treatment with ex. KCN forms a compound ‘P’. The amount of MS formed (in moles) when H$_2$S gas is passed through compound ‘P’ is:

Given below are two statements:
Statement-I: Crystal field stabilisation energy (magnitude) of $ [\text{Co}(H_2O)_6]^{2+} $ is greater than $ [\text{Ni}(H_2O)_6]^{2+} $.
Statement-II: Order of bond energy is $ \text{Cl}_2>\text{Br}_2>\text{F}_2>\text{I}_2 $.
In the light of the above statements, choose the correct option.