Redox reactions practice · Mixed difficulty

If rod of a metal (x) is put in a metal ion solution which is blue in colour, solution turn colourless. The metal rod and solution respectively are?

${Co}({s})+{Cu}^{2+}({aq}) \longrightarrow {Co}^{2+}({aq})+{Cu}({s})$

The above reaction is

In the reaction ; $2\mathrm{Ag} + 2{\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4} \to \mathrm{A}{\mathrm{g}_2}\mathrm{S}{\mathrm{O}_4} + 2{\mathrm{H}_2}\mathrm{O} + \mathrm{S}{\mathrm{O}_2},{\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}$act as :

Given below the two statements:
Statement I: The ${E^\mathrm{o}}$ value for $C{e^{4 + }}/C{e^{3 + }}$ is + 1.74 V.
Statement II: $Ce$ is more stable in $C{e^{4 + }}$ state than $C{e^{3 + }}$ state.
In the light of the above statement, choose the correct answer from the options given below:

The value of n in$\mathrm{MnO}_4^ - + 8{\mathrm{H}^ + } + n{e^ - } \to \mathrm{M}{\mathrm{n}^{2 + }} + 4{\mathrm{H}_2}\mathrm{O}$ is

Assertion: Reaction of $\mathrm{SO}_2$ and $\mathrm{H}_2 \mathrm{S}$ in the presence of $\mathrm{Fe}_2 \mathrm{O}_3$ catalyst gives element sulphur.

Reason: $\mathrm{SO}_2$ is a reducing agent.

Statement-I: Oxidation state of nitrogen in $\mathrm{N}_2 \mathrm{H}_2$ is $-1.$

Statement-II: Nitogen has fractional oxidation state in $\mathrm{N}_3 \mathrm{H}.$

What volume of 3 molar $\mathrm{HN}{\mathrm{O}_3}$ is needed to oxidise 8 g of $\mathrm{F}{\mathrm{e}^{2 + }}$ to $\mathrm{F}{\mathrm{e}^{3 + }}$ $\mathrm{HN}{\mathrm{O}_3}$, gets converted to NO :

Assertion (A): $3 {ClO}^{-} \rightarrow {ClO}_3^{-}+2 Cl^{-}$ is an example of dissociation reaction.

Reason (R): ${ClO}^{-}$ gets oxidised as well as reduced.

The eq. wt. of $\mathrm{F}{\mathrm{e}_3}{\mathrm{O}_4}$ in , $\mathrm{F}{\mathrm{e}_3}{\mathrm{O}_4} + \mathrm{KMn}{\mathrm{O}_4} \to \mathrm{F}{\mathrm{e}_2}{\mathrm{O}_3} + \mathrm{Mn}{\mathrm{O}_2}$ is:

For combustion of one mole acetone into $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}$, moles of electron transferred during redox reaction :-

Which is not a redox reaction?

How many electrons are involved in oxidation of $\mathrm{KMn}{\mathrm{O}_4}$ in basic medium?

Statement-I: In the reaction, $\frac{1}{2} \mathrm{O}_2+\mathrm{F}_2 \rightarrow \mathrm{OF}_2, \mathrm{~F}_2$ is oxidant.

Statement-II: Fluorine cannot show positive oxidation state.

When $\mathrm{KMn}{\mathrm{O}_4}$ as oxidising agent and ultimately forms $\mathrm{MnO}_4^{2 - }, \, {\text{MnO}}_{2}, \, \mathrm{M}{\mathrm{n}_2}{\mathrm{O}_3} \, \mathrm{and M}{\mathrm{n}^{2 + }},$ the number of electrons transferred per mole of $\mathrm{KMn}{\mathrm{O}_4}$ each case respectively is:

Which of the following is redox reaction

Sulphur Containing species that cannot be a reducing agent is

Assertion: $\mathrm{HNO}_2$ acts as reducing agent only.
Reason: $\mathrm{HNO}_2$ oxidises to $\mathrm{HNO}_3$ only but not reduce by any reducing agent.

Oxidation number of sodium in sodium amalgam is

The equivalent weight of element is 5.33. If it forms oxychloride which is isomorphous with ${CrO}_2 {Cl}_2$ the atomic weight of element is

Identify the set from the following sets in which all species can exhibit disproportionation reactions.

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

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

Solution of potassium chloride or ammonium nitrate in salt-bridge usually solidified by boiling with

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

The half-reactions that involve gain of electrons are known as