iCON Education - Redox Reactions TS-EAMCET Test

100 mL of $0.05 \mathrm{M} \mathrm{Cu}^{2+}$ aqueous solution is added to IL of 0.1 M KI solution. The number of moles of $\mathrm{I}_2$ and $\mathrm{Cu}_2 \mathrm{I}_2$ formed are respectively.

$2.5 \times 10^{-3}, 5 \times 10^{-3}$

$5 \times 10^{-3}, 5 \times 10^{-3}$

$5 \times 10^{-3}, 2.5 \times 10^{-3}$

$2.5 \times 10^{-3}, 2.5 \times 10^{-3}$

$ \begin{aligned} &\text { Consider the following redox reaction in basic medium. }\\ &\begin{aligned} x \mathrm{Cr}(\mathrm{OH})_3+y\left(\mathrm{IO}_3\right)^{-} & +\mathrm{z}(\mathrm{OH})^{-} \rightarrow a\left(\mathrm{CrO}_4\right)^{2-}+b(\mathrm{I})^{-}+\mathrm{c}\left(\mathrm{H}_2 \mathrm{O}\right) \end{aligned} \end{aligned} $

The incorrect option about it is

What are the products formed when ammonium dichromate is thermally decomposed?

$\mathrm{NO}_2, \mathrm{Cr}_2 \mathrm{O}_3, \mathrm{H}_2$

$\mathrm{N}_2 \mathrm{O}, \mathrm{Cr}_2 \mathrm{O}_3, \mathrm{H}_2 \mathrm{O}$

$\mathrm{N}_2, \mathrm{CrO}_3, \mathrm{H}_2 \mathrm{O}$

$\mathrm{N}_2, \mathrm{Cr}_2 \mathrm{O}_3, \mathrm{H}_2 \mathrm{O}$

In which of the following, oxidation state of nitrogen is lowest?

$\mathrm{NH}_2 \mathrm{OH}$

$\mathrm{NH}_4 \mathrm{Cl}$

$\mathrm{N}_2 \mathrm{H}_4$

The number of moles of oxalate ions oxidised by one mole of permanganate ions in acidic medium is

If the number of moles of $\mathrm{Fe}^{2+}$ ions oxidised by one mole of acidified $\mathrm{MnO}_4^{-}$is $x$, the number of moles of $\mathrm{Fe}^{2+}$ ions oxidised by one mole of acidified $\mathrm{Cr}_2 \mathrm{O}_7^{2-}$ is

In acidic medium one mole each of $\mathrm{MnO}_4^{-}$and $\mathrm{Cr}_2 \mathrm{O}_7^{2-}$ is reduce by $x$ and $y$ moles of ferrous ions. The sum of $x$ and $y$ is

$\mathrm{C}+$ Conc. $\mathrm{H}_{2} \mathrm{SO}_{4} \xrightarrow{\Delta} X+Y+\mathrm{H}_{2} \mathrm{O}$

$X$ and $Y$ in the above reaction are

$\mathrm{CO}, \mathrm{SO}_{3}$

$\mathrm{CO}_{2}, \mathrm{SO}_{2}$

$\mathrm{CO}, \mathrm{SO}_{2}$

$\mathrm{C}_{3} \mathrm{O}_{2}, \mathrm{SO}_{2}$

Observe the following reaction,

$ 2 \mathrm{KClO}_{3}(s) \xrightarrow{\Delta} 2 \mathrm{KCl}(\mathrm{~s})+3 \mathrm{O}_{2}(\mathrm{~g}) $

In this reaction

Cl is oxidised and O is reduced

Cl is reduced and O is oxidised

K is oxidised and O is reduced

K is reduced and Cl is also reduced

Match the following.

List.l (Substance)	List II (Equivalent weight)
A $\mathrm{Na}_2 \mathrm{CO}_3$	I. $\frac{M}{5}$
B $\mathrm{KMnO}_4 / \mathrm{H}^{+}$	II. $\frac{M}{3}$
C $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7 / \mathrm{H}^{+}$	III. $\frac{M}{2}$
D $\mathrm{KMnO}_4 / \mathrm{H}_2 \mathrm{O}$	IV. $\frac{M}{6}$

( $M=$ Formula weight)

The correct answer is

A-III, B-I, C-IV, D-II

A -III, B -IV, C-I, D-II

$\mathrm{A}-\mathrm{II}, \mathrm{B}-\mathrm{III}, \mathrm{C}-\mathrm{IV}, \mathrm{D}-\mathrm{I}$

A -IV, B-II, C-III, D-I

The normality of 20 volume solution of hydrogen peroxide is

In which of the following, ions are correctly arranged in the increasing order of oxidising power?

$\mathrm{Cr}_2 \mathrm{O}_7^{2-}<\mathrm{MnO}_4^{-}<\mathrm{VO}_2^{+}$

$\mathrm{VO}_2^{+}<\mathrm{Cr}_2 \mathrm{O}_7^{2-}<\mathrm{MnO}_4^{-}$

$\mathrm{VO}_2^{+}<\mathrm{MnO}_4^{-}<\mathrm{Cr}_2 \mathrm{O}_7^{2+}$

$\mathrm{MnO}_4^{-}<\mathrm{Cr}_2 \mathrm{O}_7^{2-}<\mathrm{VO}_2^{+}$

Observe the following reactions.

$ \begin{aligned} & \text { I. } \mathrm{H}_2 \mathrm{O}(l)+2 \mathrm{Na}(s) \longrightarrow 2 \mathrm{NaOH}(a q)+\mathrm{H}_2(g) \\\\ & \text { II. } 2 \mathrm{H}_2 \mathrm{O}(l)+2 \mathrm{~F}_2(g) \longrightarrow 4 \mathrm{H}^{+}(a q)+4 \mathrm{~F}^{-}(a q)+\mathrm{O}_2(g) \end{aligned} $

In both reaction I and reaction II, water is oxidised.

In both reaction I and reaction II, water is reduced.

In reaction I water is reduced and in reaction II water is oxidised.

In reaction I water is oxidised and in reaction II water is reduced.

The oxidation states of three carbon atoms in carbon suboxide $\left(\mathrm{C}_3 \mathrm{O}_2\right)$ respectively are

Which of the following reaction gives nitrogen (II) oxides as one of the products?

$\mathrm{Cu}+$ dil. $\mathrm{HNO}_3 \rightarrow$

$\mathrm{Cu}+$ conc. $\mathrm{HNO}_3 \rightarrow$

$\mathrm{Zn}+$ conc. $\mathrm{HNO}_3 \rightarrow$

Which of the following is the strongest reducing agent?

Which of the following is only a redox reaction but not a disproportionation reaction?

$4 \mathrm{H}_3 \mathrm{PO}_3 \longrightarrow 3 \mathrm{H}_3 \mathrm{PO}_4+\mathrm{PH}_3$

$2 \mathrm{H}_2 \mathrm{O}_2 \longrightarrow 2 \mathrm{H}_2 \mathrm{O}+\mathrm{O}_2$

$\mathrm{P}_4+3 \mathrm{NaOH}+3 \mathrm{H}_2 \mathrm{O} \longrightarrow 3 \mathrm{NaH}_2 \mathrm{PO}_2+\mathrm{PH}_3$

$\mathrm{P}_4+8 \mathrm{SOCl}_2 \longrightarrow 4 \mathrm{PCl}_3+2 \mathrm{~S}_2 \mathrm{Cl}_2+4 \mathrm{SO}_2$

The equivalent weight of which of the following is maximum? (Given : atomic weights $\mathrm{Na}=23, \mathrm{Mn}=55$, $ \mathrm{Cr}=52, \mathrm{~K}=39, \mathrm{O}=16, \mathrm{C}=12) $

$\mathrm{Na}_2 \mathrm{C}_2 \mathrm{O}_4 \cdot 2 \mathrm{H}_2 \mathrm{O}$

$\mathrm{KMnO}_4 / \mathrm{H}^{+}$

$\mathrm{KMnO}_4 / \mathrm{H}_2 \mathrm{O}$

$\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7 / \mathrm{H}^{+}$

Which of the following are disproportionation reactions?

(A) $\mathrm{Cl}_2+2 \mathrm{NaOH} \longrightarrow \mathrm{NaCl}+\mathrm{NaOCl}+\mathrm{H}_2 \mathrm{O}$

(B) $\mathrm{H}_2 \mathrm{O}_2 \longrightarrow 2 \mathrm{H}_2 \mathrm{O}+\mathrm{O}_2$

(D) $3 \mathrm{MnO}_4^{2-}+4 \mathrm{H}^{+} \longrightarrow 2 \mathrm{MnO}_4^{-}+\mathrm{MnO}_2+2 \mathrm{H}_2 \mathrm{O}$

The number of moles of ferrous oxalate oxidised by one mole of $\mathrm{KMnO}_4$ in acidic medium is

Identify the pair of reactions undergoing disproportionation from the following.

$ \begin{aligned} & 2 \mathrm{H}_2 \mathrm{O}_2 \longrightarrow 2 \mathrm{H}_2 \mathrm{O}+\mathrm{O}_2 \text { and } \\ & \mathrm{Cl}_2+2 \mathrm{NaOH} \longrightarrow \mathrm{NaCl}+\mathrm{NaOCl}+\mathrm{H}_2 \mathrm{O} \end{aligned} $

$ \begin{aligned} & \mathrm{P}_4+3 \mathrm{NaOH}+3 \mathrm{H}_2 \mathrm{O} \longrightarrow \mathrm{PH}_3+3 \mathrm{NaH}_2 \mathrm{PO}_4 \\ & \text { and } \mathrm{Cl}_2+2 \mathrm{Na} \longrightarrow 2 \mathrm{NaCl} \end{aligned} $

$ \begin{aligned} & \mathrm{Cl}_2+2 \mathrm{KBr} \longrightarrow 2 \mathrm{KCl}+\mathrm{Br}_2 \text { and } \\ & 5 \mathrm{Cl}_2+\mathrm{I}_2+6 \mathrm{H}_2 \mathrm{O} \longrightarrow 2 \mathrm{IO}_3^{-}+10 \mathrm{Cl}^{-}+2 \mathrm{H}^{+} \end{aligned} $

$ \begin{aligned} & \mathrm{Pb}_3 \mathrm{O}_4+8 \mathrm{HCl} \longrightarrow 3 \mathrm{PbCl}_2+\mathrm{Cl}_2+\mathrm{H}_2 \mathrm{O} \text { and } \\ & \mathrm{P}_4+3 \mathrm{NaOH} \longrightarrow 3 \mathrm{H}_2 \mathrm{O}+\mathrm{PH}_3+3 \mathrm{NaH}_2 \mathrm{PO}_4 \end{aligned} $

The weight of potassium dichromate (molecular weight $=294$ ) required to prepare 0.04 N of 250 mL solution is

What is the equivalent weight of $\mathrm{KMnO}_4$ in acidic medium? (Molecular weight of $\mathrm{KMnO}_4=158 \mathrm{~g}$ )

$\mathrm{KMnO}_4$ oxidises $\mathrm{C}_2 \mathrm{H}_2 \mathrm{O}_4$ to form $\mathrm{CO}_2$. In which of the following, the reaction will be faster?

$A q . \mathrm{HCl}$ solution

Aq. $\mathrm{NaHCO}_3$, solution