Balance the following equation by ion-electron method In acidic medium.
\(Mn{O}_4^-+I^-\rightarrow MnO_2+I_2\)

Balance the following equation by ion-electron method In acidic medium.
\(Mn{O}_4^-+Fe^{2+}\rightarrow Mn^{2+}+Fe^{3+}\)

Balance the following equation by ion-electron method In acidic medium.
\(Cr{(OH)}_4^-+H_2O_2\rightarrow Cr{O}_4^{2-}\)

(a) Define equivalent mass of an oxidising agent.
(b) How would you calculate the equivalent mass of potassium permanganate?

(a) Define equivalent mass of an reducing agent.
(b) How would you determine the equivalent mass of Ferrous sulphate?

A compound on analysis gave the following percentage composition: C = 24.47%, H = 4.07 %, CI = 71.65%. Find out its empirical formula.

A laboratory analysis of an organic compound gives the following mass percentage composition: C = 60%, H = 4.48% and remaining oxygen.

An insecticide has the following percentage composition by mass: 47.5% C, 2.54% H, and 50.0% Cl. Determine its empirical formula and molecular formulae. Molar mass of the substance is 354.5g mol^-1

Calculate the percentage composition of the elements present in magnesium carbonate. How many Kg of CO₂ can be obtained from 100 Kg of is 90% pure magnesium carbonate.

Urea is prepared by the reaction between ammonia and carbon dioxide.
2NH_3(g) + CO_2(g) → (NH₄)₂CO_(ag) + H₂O_(I)
In one process, 637.2 g of NH₃ are allowed to react with 1142 g of CO₂
(a) Which of the two reactants is the limiting reagent?
(b) Calculate the mass of (NH₄)₂CO formed.
(c) How much of the excess reagent in grams is left at the end of the reaction? 

(a) Define oxidation number.
(b) What are the rules used to assign oxidation number ?

Balance the following equation by oxidation number method.
C₆H₆ + O₂\(\rightarrow\)CO₂ + H₂O

Balance the following equation by oxidation number method.
KMnO₄ + HCI \(\rightarrow\) KCl + MnCl₂ + H₂O + Cl₂

Explain the steps involved in ion-electron method for balancing redox reaction.

Define the following
(a) equivalent mass of an acid
(b) equivalent mass of a base
(c) equivalent mass of an oxidising agent
(d) equivalent mass of a reducing agent.

Balance the following equation by oxidation number method.
KMnO₄ + FeSO₄ + H₂SO₄ \(\rightarrow\)K₂SO₄ + MnSO₄ + Fe₂(SO₄)₃ + H₂O

Balancing of the molecular equation in alkaline medium. 
MnO₂ + O₂ + KOH\(\rightarrow\)K₂MnO₄ + H₂O

Write balanced equation for the oxidation of Ferrous ions to Ferric ions by permanganate ions in acid solution. The permanganate ion forms Mn²⁺ ions under these conditions.

A flask A contains 0.5 mole of oxygen gas. Another flask B contains 0.4 mole of ozone gas. Which of the two flasks contains greater number of oxygen atoms.

(a) Formulate possible compounds of 'CI' in its oxidation state is: 0, -1, +1, +3, +5, +7
(b) H₂O₂ act as an oxidising agent as well as reducing agent where as O₃ act as only oxidizing agent. Prove it.

The Mn³⁺ ion is unstable in solution and undergoes disproportionation to give Mn²⁺, MnO₂ and H⁺ ion. Write a balanced ionic equation for the reaction.

Chlorine is used to purify drinking water. Excess of chlorine is harmful. The excess chlorine is removed by treating with sulphur dioxide. Present a balanced equation for the reaction for this redox change taking place in water.

\({ 2NH }_{ 3 }\left( g \right) +{ CO }_{ 2 }\left( g \right) \rightarrow \underset{Urea}{H_2N}-\overset { \underset { || }{ O } }{ C } -{ NH }_{ 2 }\left( aq \right) +{ H }_{ 2 }O(I)\)
In a process, 646 g of ammonia is allowed to react with 1.144 kg of CO₂ to form urea.
(i) If the entire quantity of all the reactants is not consumed in the reaction which is the limiting reagent ?
(ii) Calculate the quantity of urea formed and unreacted quantity of the excess reagent. The balanced equation is 
\(\overset { { 2NH }_{ 3 }+{ CO }_{ 2 } }{ \underset { { H }_{ 2 }NCON{ H }_{ 2 }+{ H }_{ 2 }O }{ \downarrow } } \)