Science (English Medium) Class 11 - CBSE Question Bank Solutions for Chemistry

Describe the effect of Removal of CO on the equilibrium of the reaction: 

\[\ce{2H2(g) + CO (g) ⇌ CH3OH (g)}\]

Describe the effect of Removal of CH₃OH on the equilibrium of the reaction:

\[\ce{2H2(g) + CO (g) ⇌ CH3OH (g)}\]

Among NH₃, H₂O and HF, which would you expect to have highest magnitude of hydrogen bonding and why?

Arrange the following:

CaH₂, BeH₂ and TiH₂ in order of increasing electrical conductance.

Describe the usefulness of water in biosphere and biological systems.

What properties of water make it useful as a solvent? What types of compound can it (i) dissolve, and (ii) hydrolyse?

Dihydrogen gas used in Haber’s process is produced by reacting methane from natural gas with high-temperature steam. The first stage of two-stage reaction involves the formation of CO and H₂. In the second stage, CO formed in the first stage is reacted with more steam in water gas shift reaction,

\[\ce{CO (g) + H2O (g) ⇌ CO2 (g) + H2 (g)}\]

If a reaction vessel at 400°C is charged with an equimolar mixture of CO and steam such that `"p"_"CO" = "p"_("H"_2"O")` = 4.0 bar, what will be the partial pressure of H₂ at equilibrium? K_p = 10.1 at 400°C.

The statement that is not correct for periodic classification of elements is ______.

All transition elements are d-block elements, but all d-block elements are not transition elements. Explain

In which of the following molecule/ion all the bonds are not equal?

Which of the following statements are correct about \[\ce{CO^{2-}3}\]?

(i) The hybridisation of central atom is sp³.

(ii) Its resonance structure has one \[\ce{C - O}\] single bond and two \[\ce{C = O}\] double bonds.

(iii) The average formal charge on each oxygen atom is 0.67 units.

(iv) All \[\ce{C - O}\] bond lengths are equal.

All the \[\ce{C - O}\] bonds in carbonate ion \[\ce{(CO^{2-}3)}\] are equal in length. Explain.

Describe hybridisation in the case of \[\ce{PCl5}\] and \[\ce{SF6}\]. The axial bonds are longer as compared to equatorial bonds in \[\ce{PCl5}\] whereas in \[\ce{SF6}\] both axial bonds and equatorial bonds have the same bond length. Explain.

Which of the following arrangements represent increasing oxidation number of the central atom?

Assertion (A): Among halogens fluorine is the best oxidant.

Reason (R): Fluorine is the most electronegative atom.

Assertion (A): In the reaction between potassium permanganate and potassium iodide, permanganate ions act as oxidising agent.

Reason (R): Oxidation state of manganese changes from +2 to +7 during the reaction.

Which of the following equations depict the oxidising nature of \[\ce{H2O2}\]?

Which of the following equation depicts reducing nature of \[\ce{H2O2}\]?

Some of the properties of water are described below. Which of them is/are not correct?

(i) Water is known to be a universal solvent.

(ii) Hydrogen bonding is present to a large extent in liquid water.

(iii) There is no hydrogen bonding in the frozen state of water.

(iv) Frozen water is heavier than liquid water.

If same mass of liquid water and a piece of ice is taken, then why is the density of ice less than that of liquid water?