Types of Redox Reactions

Q. 18. For dissociation reaction:N2O4(g)=2NO2(g), the degree of dissociation in terms of Kp and total equilibrium pressure P??

Q.

The order of ionization enthalpy for B, Al and Ga is:

1. B<Al<Ga

2. Ga<Al<B

3. B>Al>Ga

4. B>Al<Ga

Q.

The reaction, $3Cl{O}^{-}\left(aq\right)⟶Cl{O}_3^{-}\left(aq\right)+2C{l}^{-}\left(aq\right)$ is an example of:

1. Oxidation reaction

2. Reduction reaction

3. Disproportionation Reaction

4. Decomposition reaction

Q.

In the oxidation of ${\mathrm{N}}_2{\mathrm{H}}_4$to ${\mathrm{N}}_2$, Equivalent weight of ${\mathrm{N}}_2{\mathrm{H}}_4$ would be________

Q. In acidic medium, dichromate ions oxidise ferrous sulphate to ferric sulphate and itself gets reduced to Cr3+ ions. Write a balanced equation to represent this redox reaction.(Use ion electron method)

Q.

Which one of the following pair of substances illustrate the law of multiple proportions?

1. H₂ and D₂

2. SO₂ and SO₃

3. BaO and Ba(OH)₂

4. KCl and KBr

Q.

Presence of particulate matter in polluted air catalyses the oxidation of sulphur dioxide to:

1. Nitric oxide

2. Hydrogen peroxide

3. Dioxygen

4. Sulphur trioxide

Q. the molar concentration of H+ ion when 0.1M of 200 ml HCl is mixed with 0.05 M of 300 ml H2SO4 is

Q.

Which of the following process does NOT occur during a chemical reaction?

1. Collision between molecules

2. Rearrangement of atoms

3. Formation of new products from the elements that are not present in the reactants

4. Formation of new atoms

Q. 7. Equivalent Weight of K2Cr2O7 in the reaction K2Cr2O7→ K2CrO4 + Cr2O3 + O2.??

Q.

0.5g of an organic compound on kjeldhal's analysis gave enough ammonia to just neutralize 10cm3 of 1M $H_{2}S{O}_4$. The $\%$of nitrogen in the compound is

1. 56

2. 28

3. 42

4. 14

Q. Q 36/90 100 ml of 0.2 M Na2SO4 solution is mixedwith 400 ml of 0.1 M Al2(SO4)3 solution. The molarconcentration of SO42 ion in the final solution is

Q. if hydration enthalpy is measured in terms of no of water molecules surrounding the ion in the solution. then why is lithium heavily hydrated when small size of ion can surround only few water molecules ?

Q. Pl. explain the law of multiple proportions, with an example and explain the example accordingly.

Q. In preparation of hydrogen from zinc why is hydrogen passed through silver nitrate and lead nitrate solution

Q. Do all the peroxides and superoxides of alkali metals behave as good oxidising agent without any exceptions ?

Q. 2 he correct order of ionisation potential of Na, P, Cl is

Q. Why is phenopthalein not used as an indicator in the titration of weak acid and strong base ?

Q.

Which law is also known as Law of constant composition?

1. Law of multiple proportions

2. Avogadro's law

3. Law of definite proportions

4. Law of conservation of mass

Q. Which of the following is correct formula for calculation of n factor for disproportionation reaction.

1. $n_f=(n_f{)}_{\text{oxidation}}+(n_f{)}_{\text{reduction}}$
2. $\frac{1}{n_f}=\frac{1}{(n_f{)}_{\text{oxidation}}}+\frac{1}{(n_f{)}_{\text{reduction}}}$
3. $n_f=(n_f{)}_{\text{oxidation}}^2+(n_f{)}_{\text{reduction}}^2$
4. None of these.

Q. Balance the following equation in basic medium by ion-electron method and oxidation number method and identify the oxidising agent and the reducing agent.

Q. 77. 25 ml of a solution containing NaOH and Na2CO3(sodium bi carbonate) required (1) 50 ml of 0.2 N HCl using phenolphthalein as an indicator (2) 72 ml of 0.2N HCl when titrated using methyl orange as an indicator. The ratio of weight of NaOH and Na2CO3 in the solution is (1) 0.48 (2)0.44 (3)0.40 (4)0.38

Q. Why is phenopthalein not used as an indicator in the titration of weak acid and strong base ?

Q. Why does acidic character increases down the group in case of reaction of group 15 elements with hydrogen and decreases down the group in case of reaction of group 15 with oxygen? Kindly explain.

Q. In Haber's process, the equivalent weight of nitrogen gas is:

1. $\frac{M}{3}$
2. $3M$
3. $\frac{M}{6}$
4. $M$

Q. A sample of $FeS{O}_4$ and $Fe{C}_2{O}_4$ is dissolved in $H_{2}S{O}_4$. The complete oxidation of sample required 8/3 eqv. of $KMn{O}_4$. After oxidation, the reaction mixture was reduced by $Zn$. On further oxidation by $KMn{O}_4$ 5/3 eqv were used. The moles of $Fe{C}_2{O}_4$ in the mixture is

Q. The concentration of \lbrack H^+\rbrack and concentration of \lbrack OH^-\rbrack of a 0.1 M aqueous solution of 2% ionised weak acid is ionic product of water=10^{-14})

Q. Identify the substances oxidised, reduced, oxidising agent and reducing agent for the given reaction-

Q. During the disproportionation of Iodine to iodide and iodate ions, the ratio of iodate and iodide ions formed in alkaline medium is:

$I_2\to I{O}_3^{-}+I^{-}$

1. 1 : 5
2. 5 : 1
3. 3 : 1
4. 1 : 3

Q.

Which of the following mixture present in water acts as a good buffer?

1. 0.07 mole HCN, 0.02 mole KCN

2. 0.03 mole HCN, 0.06 mole KCN

3. 0.02 mole HCN, 0.03 mole KCN

4. 0.07 mole HCN, 0.06 mole KCN