Download App

Equilibrium — Chemistry STD 11 Science — Question

Rajasthan BoardEnglish MediumSTD 11 ScienceChemistryEquilibrium3 Marks
Question
Some processes are given below. What happens to the process if it is subjected to a change given in the brackets?

  1.  

(Pressure is increased)

  1. Dissolution of NaOH in water (Temperature is increased.)
  2. $\text{N}_2(\text{g})+\text{O}_2(\text{g})\rightleftharpoons2\text{NO}(\text{g})-180.7\text{KJ}$ (Pressure is increased and temperature is decreased.)
✓

Answer

  1. Equilibrium will shift in the forward direction, i.e. more of ice will melt.
  2. Solubility will decrease because it is an exothermic process.
  3. Pressure has no effect. Decrease of temperature will shift the equilibrium in the backward direction.

Need a full question paper?

Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.

Start Generating Free

Explore more

More "3 Marks Question" from Equilibrium→Equilibrium — all question types→Chemistry STD 11 Science question papers→Rajasthan Board STD 11 Science question papers→Rajasthan Board question paper generator→

Similar questions

Using molecular orbital theory, compare the bond energy and magnetic character of O+2 and O–2.
→
The following techniques are used to quantitatively estimate extra elements in organic compound. Identify the name of the method and the element estimated by this method.
  1. A known mass of an organic compound is heated with fuming HNO3 in presence of AgNO3.
  2. Organic compound is heated with dry copper oxide in atmosphere of CO2.
  3. Organic compound is heated with conc. H2SO4.
→
If 2 litres of N2 is mixed with 2 litres of H2 at a constant temperature and pressure, then what will be the volume of NH3 formed?
→
Calculate the amount of carbon dioxide that could be produced when
(i) 1 mole of carbon is burnt in air.
(ii) 1 mole of carbon is burnt is 16 g of dioxygen.
(iii) 2 moles of carbon are burnt in 16 g of dioxygen.
→
Justify the following statements.
  1. Reactions with $\Delta\text{G}<0$ always have an equilibrium constant greater than 1.
  2. Many thermodynamically feasible reactions do not occur under ordinary conditions.
  3. At low temperatures, enthalpy change dominates the $\Delta\text{G}$ expression and at high temperatures, it is the entropy which dominates the value of $\Delta\text{G}.$
→
Suggest a method to purify:
  1. Camphor containing traces of common salt.
  2. Kerosene oil containing water.
  3. A liquid which decomposes at its boiling point.
→
Note: Consider structures I to VII and answer the questions:

  1. $\text{CH}_3-\text{CH}_2-\text{CH}_2-\text{CH}_2-\text{OH}$

  2. $\text{CH}_3-\text{CH}_2-\text{CH}-\text{CH}_3\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ |\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{OH}$

  3. $\ \ \ \ \ \ \ \ \ \ \ \ \text{CH}_3\\\ \ \ \ \ \ \ \ \ \ \ \ \ |\\\text{CH}_3-\text{C}-\text{CH}_3\\\ \ \ \ \ \ \ \ \ \ \ \ \ |\\\ \ \ \ \ \ \ \ \ \ \ \ \text{OH}$

  4. $\text{CH}_3-\text{CH}-\text{CH}_2-\text{OH}\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ |\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{CH}_3$

  5. $\text{CH}_3-\text{CH}_2-\text{O}-\text{CH}_2-\text{CH}_3$

  6. $\text{CH}_3-\text{O}-\text{CH}_2-\text{CH}_2-\text{CH}_3$

  7. $\text{CH}_3-\text{O}-\text{CH}-\text{CH}_3\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ |\\\ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \ \text{CH}_3$

Identify the pairs of compounds that represents position isomerism.

→
Complete the reactions:
  1. $\text{CH}_3\text{CH}_2\text{CH}_3+\text{HNO}_3\xrightarrow{\text{Vapour phase}}$
  2. $\text{CH}_4+\text{O}_2\xrightarrow[723-773\text{K}]{\text{Copper tube}}$
  3. $\text{C}_2\text{H}_5\stackrel{{\ \ \ \ \ \ \ \ \ -}}{\hbox{COO} }\stackrel{{+}}{\hbox{Na}}+\text{NaOH}\xrightarrow{\text{CaO}}$
→
What is meant by the term bond order? Calculate the bond order of $\text{N}_2,\text{O}_2,\text{O}^+_2$ and $\text{O}^-_2.$
→
  1. Define Aufbau's principle.
  2. Draw the shape of $\text{d}_{\text{z}^2}$ orbital.
  3. Which quantum number specify number of orbitals in a given subshell?
→