List of top Chemistry Questions on Oxidation-Reduction

\[ S_2O_3^{2-}(aq) + OH^{-}(aq) \rightarrow SO_4^{2-}(aq) + H_2O(l) + e^{-} \]
After the above half reaction is balanced, which of the following are the coefficients of $OH^{-}$ and $SO_4^{2-}$ respectively?

$\Delta G^\circ$ (in kJ mol$^{-1}$) for the cell reaction given below is \[ 2Al(s)+3Cu^{2+}(aq)\rightarrow 2Al^{3+}(aq)+3Cu(s) \] \[ \text{Given: }E^\circ_{Al^{3+}/Al}=-1.66V,\quad E^\circ_{Cu^{2+}/Cu}=+0.34V,\quad F=96500\;C\,mol^{-1} \]

Molten $Al_2O_3$ was electrolyzed between carbon electrodes. The mass (in g) of aluminium produced at cathode when 965 amperes current is passed through it for 1000 seconds is ($F=96500\,C\,mol^{-1}$)

$\text{KMnO}_4$ oxidizes $\text{M}^{2+}$ to $\text{M}^{4+}$ in acid medium. $500\text{ mL}$ of $0.02\text{M}$ $\text{M}^{2+}$ solution requires $500\text{ mL}$ of $x\text{ M}$ $\text{MnO}_4^-$ solution for complete oxidation. The value of $x$ is:

$E_{cell}$, for the cell given below is 0.82 V. What is its $E^{\circ}$ value? $Fe | Fe^{2+}(0.001 \text{ M}) || Cu^{2+}(0.1 \text{ M}) | Cu$. (Given: $\frac{2.303 RT}{F} = 0.06 \text{ V}$)

The value of $log K_{c}$ for the given cell reaction at 298 K is
$Cu(s)+2Ag^{+}(aq)\rightarrow Cu^{2+}(aq)+2Ag(s)$.
(Given: $E^{\circ}_{Cu^{2+}/Cu}=0.34V, E^{\circ}_{Ag^{+}/Ag}=0.80V; \frac{2.303RT}{F}=0.06$)

The number of moles of $H_{2}$ gas liberated at cathode, when 10 mA current is passed through dilute NaCl for $19.3 \times 10^{4}$ seconds is ($F=96500 C mol^{-1}$)

Observe the following unbalanced equation $aS_{8}+b~OH^{-}(aq)\rightarrow cS^{2-}(aq)+dS_{2}O_{3}^{2-}(aq)+eH_{2}O(l)$. In the balanced equation, the ratio of c and d is:

The number of Faradays involved in the conversion of 0.25 mol of $Al^{3+}$ to Al is x and number of Faradays involved in the conversion of 1100 mL of 0.5 M $Cu^{2+}$ to Cu is y. The values of x and y respectively are:

At 298 K, $E^{\circ}$ value of the cell involving $2 Fe^{3+}(aq) + 2 I^-(aq) \rightarrow 2 Fe^{2+}(aq) + I_2(s)$ is X V. The X (in V) and $\log K_c$ for the reaction are respectively: ($E^{\circ}_{Fe^{3+}/Fe^{2+}} = 0.77$ V, $E^{\circ}_{I_2/I^-} = 0.54$ V)

The reduction products formed when copper and zinc metals are separately oxidised with dilute $HNO_{3}$ respectively are

Consider the following compounds: $H_{3}PO_{2}, Se_{2}Cl_{2}, HNO_{2}, HNO_{3}, H_{2}SO_{4}, H_{2}O_{2}$ How many of the above compounds undergo disproportionation reaction?

X, Y and Z represent three electrodes $Al^{3+}/Al$, $Cu^{2+}/Cu$ and $Ag^{+}/Ag$ with $E^{\circ}$ values -1.66, 0.34 and 0.80 V respectively. The correct order of oxidising power of these three electrodes is

Given below are two statements: Statement I: The electrical conductivity of a solution decreases with dilution. Statement II: The overall reaction in $H_{2}-O_{2}$ fuel cell is: $2H_{2}O(l)\longrightarrow2H_{2}(g)+O_{2}(g)$. The correct answer is:

According to Faraday's first law of electrolysis, the mass of substance deposited ($w$) is proportional to

Oxidation state of each Cl in CaOCl is/are

Which of these will not be oxidized by ozone?

What are the oxidation states of three Br atoms in $Br_3O_8$ molecule