Redox reactions practice · Medium

${C}_2 {H}_6(g)+{NO}_2(g) \rightarrow {CO}_2(g)+{H}_2 {O}(l)$

In this equation, the ratio of the coefficients of ${CO}_2$ and ${H}_2 {O}$ is

The oxidation number of $\mathrm{Ni}$ in ${\mathrm{K}_4}\left[ {\mathrm{Ni}{{\left( {\mathrm{CN}} \right)}_4}} \right]$ is :

Chlorine undergoes disproportionation in alkaline medium as shown below :
$a \mathrm{Cl}_{2(g)}+b O H_{(a q)}^{-} \rightarrow \mathrm{cClO}_{(a q)}^{-}+d \mathrm{Cl}_{(a q)}^{-}+\mathrm{eH}_2 \mathrm{O}_{(l)}$

The values of $\mathrm{a}, \mathrm{b}, \mathrm{c}$ and $\mathrm{d}$ in a balanced redox reaction are respectively:

In the reactions;$\mathrm{A}{\mathrm{s}_2}{\mathrm{S}_3} + \mathrm{HN}{\mathrm{O}_3} \to {\mathrm{H}_3}\mathrm{As}{\mathrm{O}_4} + {\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4} + \mathrm{NO}$, the element oxidized is/ are :

In which compound, oxygen has an oxidation state of $+ 2$ ?

Oxidation state of $\mathrm{P}$ in $\mathrm{H}_4 \mathrm{P}_2 \mathrm{O}_5, \mathrm{H}_4 \mathrm{P}_2 \mathrm{O}_6$ and $\mathrm{H}_4 \mathrm{P}_2 \mathrm{O}_7$ are respectively :

Among the properties given below, the set of properties shown by $\mathrm{C}{\mathrm{N}^ - }$ ion towards metal species is :1. Reducing; 2. Oxidising ; 3. Complexation

In the reaction, $\mathrm{NaH} + {\mathrm{H}_2}\mathrm{O} \to \mathrm{NaOH} + {\mathrm{H}_2}$:

Statement-I: $\mathrm{H}_2 \mathrm{SO}_4$ can act as reducing agent and oxidising agent.

Statement-II: Sulphur can not increase its oxidation number beyond +6.

Which of the following is not a redox reaction?

Number of moles of $\mathrm{MnO}_4^ -$ required to oxidise one mole of ferrous oxalate completely in acidic medium will be :

For reducing one mole of $\mathrm{F}{\mathrm{e}^{2 + }}$ion to $Fe$, the number of faraday of electricity is :

Assertion: Among $\mathrm{Br}^-, \mathrm{O}_2^{2-}, \mathrm{H}^-$ and $\mathrm{NO}_3^-,$ the ions that could not act as oxidising agents are $\mathrm{Br}^{-}$and $\mathrm{H}^{-}.$

Reason: $\mathrm{Br}^{\ominus}$ and $\mathrm{H}^{-}$ could not be reduced.

The reaction; ${\mathrm{H}_2}\mathrm{S} + {\mathrm{H}_2}{\mathrm{O}_2} \to 2{\mathrm{H}_2}\mathrm{O} + \mathrm{S}$ shows :

Statement-I: ${KClO}_3 \rightarrow {KClO}_4+{KCl}$. This is a disproportionation reaction.
Statement-II: The reaction in which one substance gets oxidised and reduced is known as disproportionation reaction.

Oxidation number of carbon in carbon sub oxide $\left( {{\mathbf{C}_\mathbf{3}}{\mathbf{O}_\mathbf{2}}} \right)$

$\mathrm{Cr}_2 \mathrm{O}_7^{2-}$ is not a self indicator but

The maximum oxidation state of oxygen is

A solution of sulphur dioxide in water reacts with ${H}_2 {S}$ precipitating sulphur. Here sulphur dioxide acts as

Assertion: ${KCl} / {NaCl} / {NH}_4 {Cl}$ etc. cannot be used in the salt bridge of a cell containing silver.

Reason: A salt bridge contains concentrated solution of an inert electrolyte like ${KCl}, {KNO}_3, {NH}_4 {NO}_3$ etc. or solidified solution of such as electrolyte in agar-agar and gelatine.

Consider the following reaction, $xMnO_4^ - + y{C_2}O_4^{2 - } + z{H^ + } \to xM{n^{2 + }} + 2yC{O_2} + \frac{z}{2}{H_2}O$ The values of $x$, $y$ and $z$ in the reaction are respectively

In which reaction is hydrogen acting as an oxidising agent?

Which of the following involves transfer of five electrons?

Given below are two statements.
One is labelled as Assertion (A) and the other is labelled as Reason (R).
Assertion (A) Aluminium is extracted from bauxite by the electrolysis of molten mixture of $A{l_2}{O_3}$ with cryolite.
Reason (R) The oxidation state of $Al$ in cryolite is +3.
In the light of the above statements, choose the most appropriate answer from the options given below.

Which of the following is not a redox reaction?

Which of the following is not an intramolecular redox reaction?

Oxalic acid on reacting with acidified $\mathrm{KMn}{\mathrm{O}_4}$ is oxidised to :

In the balanced reaction, $IO_3^ - + S{O_2} + 4{H_2}O \to {I_2} + SO_4^{ - 2} + 8{H^ + }$ the coefficient of $S{O_2}$ is

Oxidation number of carbon in$\mathrm{KCN}$ is :

The value of 'n' in the reaction $\mathrm{C}{\mathrm{r}_2}\mathrm{O}_7^{2 - } + 14{\mathrm{H}^ + } + n\mathrm{F}{\mathrm{e}^{2 + }} \to 2\mathrm{C}{\mathrm{r}^{3 + }} + n\mathrm{F}{\mathrm{e}^{3 + }} + 7{\mathrm{H}^2}\mathrm{O}$ will be