Which one of the following statements is correct when \ce{SO2} is passed through acidified \ce{K2Cr2O7} solution?
Hot concentrated sulphuric acid is a moderately strong oxidizing agent. Which of the following reactions does not show oxidizing behaviour?
It is because of inability of $ns^2$ electrons of the valence shell to participate in bonding that
Name the gas that can readily decolourise acidified \ce{KMnO4} solution:
The correct order of N-compounds in their decreasing order of oxidation states is
Consider the change in oxidation state of bromine corresponding to different $E^\circ$ values as shown in the Latimer diagram below: \ce{BrO4^-} $\xrightarrow{1.82\,\text{V}}$ \ce{BrO3^-} $\xrightarrow{1.5\,\text{V}}$ \ce{HBrO} $\xrightarrow{1.595\,\text{V}}$ \ce{Br2} $\xrightarrow{1.0652\,\text{V}}$ \ce{Br^-} Then the species undergoing disproportionation is
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For the redox reaction \ce{MnO4^- + C2O4^2- + H^+ -> Mn^2+ + CO2 + H2O}, the correct coefficients of the reactants for the balanced equation are (\ce{MnO4^-}, \ce{C2O4^2-}, \ce{H^+} respectively)
Which of the following reactions are disproportionation reactions? (a) \ce{2Cu^+ -> Cu^2+ + Cu} (b) \ce{3MnO4^2- + 4H^+ -> 2MnO4^- + MnO2 + 2H2O} (c) \ce{2KMnO4 -> K2MnO4 + MnO2 + O2} (d) \ce{2MnO4^- + 3Mn^2+ + 2H2O -> 5MnO2 + 4H^+} Select the correct option from the following.
Which of the following oxoacids of phosphorus has the strongest reducing property?
When neutral or faintly alkaline \ce{KMnO4} is treated with potassium iodide, iodide ion is converted into 'X'. 'X' is
The oxidation state of \ce{Cr} in \ce{CrO5} is
The standard electrode potential ($E^\circ$) values of \ce{Al^3+/Al}, \ce{Ag+/Ag}, \ce{K+/K} and \ce{Cr^3+/Cr} are $-1.66$ V, $0.80$ V, $-2.93$ V and $-0.74$ V, respectively. The correct decreasing order of reducing power of the metals is
What is the change in oxidation number of carbon in the following reaction? \ce{CH4(g) + 4Cl2(g) -> CCl4(l) + 4HCl(g)}
Which of the following reactions is a metal displacement reaction? Choose the right option.
Identify the incorrect statement from the following:
Given below are half-cell reactions: \ce{MnO4^- + 8H^+ + 5e^- -> Mn^2+ + 4H2O}, $E^\circ_{(\ce{MnO4^-}/\ce{Mn^2+})} = -1.510$ V; \ce{1/2 O2 + 2H^+ + 2e^- -> H2O}, $E^\circ_{(\ce{O2}/\ce{H2O})} = +1.223$ V. Will the permanganate ion \ce{MnO4^-} liberate \ce{O2} from water in the presence of an acid?
In the neutral or faintly alkaline medium, \ce{KMnO4} oxidises iodide into iodate. The change in oxidation state of manganese in this reaction is from:
On balancing the given redox reaction, the coefficients $a$, $b$ and $c$ are found to be, respectively: \ce{$a$ Cr2O7^2-(aq) + $b$ SO3^2-(aq) + $c$ H^+(aq) -> 2Cr^3+(aq) + $b$ SO4^2-(aq) + $c$/2 H2O(l)}
The $E^\circ$ values are: \ce{Al+/Al} $= +0.55$ V, \ce{Tl+/Tl} $= -0.34$ V, \ce{Al^3+/Al} $= -1.66$ V and \ce{Tl^3+/Tl} $= +1.26$ V. Identify the incorrect statement.
The correct option for a redox couple is
Which reaction is NOT a redox reaction?
Consider the following compounds: \ce{KO2}, \ce{H2O2} and \ce{H2SO4}. The oxidation states of the underlined elements (\ce{K} in \ce{KO2}, \ce{O} in \ce{H2O2}, \ce{S} in \ce{H2SO4}) in them are, respectively,
The correct decreasing order of oxidation state of the underlined atom in each molecule is:
In acidic medium, $10\,$mL of $0.25\,$M oxalic acid is titrated with $\ce{KMnO4}$ solution. If the volume of $\ce{KMnO4}$ required to reach the end point is $10\,$mL, the strength of the $\ce{KMnO4}$ solution is:
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