Redox Reactions

Reaction of PtF6 with oxygen (O2) gas results in the formation of an ionic compound, X+Y-.Correct statement(s) is(are)

One of the products formed from the reaction of permanganate ion with iodide ion in neutral aqueous medium is

Ozonolysis of ClO2 produces an oxide of chlorine. The average oxidation state of chlorine in this oxide is __________.

A sample (5.6 g) containing iron is completely dissolved in cold dilute HCl to prepare a 250 mL of solution. Titration of 25.0 mL of this solution requires 12.5 mL of 0.03 M KMnO4 solution to reach the end point. Number of moles of Fe2+ pre...

A sample (5.6 g) containing iron is completely dissolved in cold dilute HCl to prepare a 250 mL of solution. Titration of 25.0 mL of this solution requires 12.5 mL of 0.03 M KMnO4 solution to reach the end point. Number of moles of Fe2+ pre...

Choose the correct statement(s) among the following :

The order of the oxidation state of the phosphorous atom in
\({H_3}P{O_2},{H_3}P{O_4},{H_3}P{O_3}\) and \({H_4}{P_2}{O_6}\) is

In neutral or faintly alkaline solution, 8 moles of permanganate anion quantitative oxidise thiosulphate anions to produce X moles of a sulphur containing product. The magnitude of X is....

Fe3+ is reduced to Fe2+ by using

Consider the following list of reagents, acidified K2Cr2O7, alkaline KMnO4, CuSO4, H2O2, Cl2, O3, FeCl3, HNO3 and Na2S2O3. The total number of reagents that can oxidise aqueous iodide to iodine is

For the reaction,\({I^ - } + ClO_3^ - + {H_2}S{O_4} \to C{l^ - } + HSO_4^ - + {I_2}\)the correct statement(s) in the balanced equation is/are

Reduction of the metal centre in aqueous permanganate ion involves

The difference in the oxidation numbers of the two types of sulphur atoms in Na2S4O6 is

Match the reactions in Column I with nature of the reactions/type of the products in Column II. Indicate your answer by darkening the appropriate bubbles of the 4 \(\times\) 4 matrix given in the ORS.

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The reaction, \(3Cl{O^ - }(aq)\)\(\to ClO_3^ - (aq) + 2C{l^ - }(aq)\) is an example of :

Amongst the following identify the species with an atom in +6 oxidation state

The normality of 0.3 M phosphorus acid (H3PO3) is

To a 25ml H2O2 solution, excess of acidified solution of potassium iodide was added. The iodine liberated required 20 ml of 0.3 N sodium thiosulphate solution. Calculate the volume strength of H2O2 solution.

A 5.0 cm3 solution of H2O2 liberates 0.508 g of iodine from an acidified KI solution. Calculate the strength of H2O2 solution in terms of volume strength at STP.

For the redox reaction:
\(MnO_4^ - + {C_2}O_4^{ - 2} + {H^ + }\) \(\to M{n^{2 + }} + C{O_2} + {H_2}O\)
The correct coefficients of the reactants for the balanced
reaction are

The volume strength of 1.5 N H2O2 solution is

The oxidation number of phosphorus in Ba(H2PO2) is :

The equivalent weight of MnSO4 is half of its molecular weight, when it converts to

Complete and balance the following equation:
S + OH- \(\to\) S2- + \(S_2O_3^-\)

Complete and balance the following equation:
\(ClO_3^-\) + I- + H2SO4 \(\to\) Cl- + \(HSO_4^-\)

Arrange the following in increasing oxidation number of iodine.
I2, HI, HIO4, ICl

Complete and balance the following equation:
Ag+ + AsH3 \(\to\) H3AsO3 + H+

Complete and balance the following equation:
Mn2+ + PbO2 \(\to\) \(MnO_4^-\) + H2O

Complete and balance the following equation:
HNO3 + HCl \(\to\) NO + Cl2

Complete and balance the following equation:
\(Cr_2O_7^{2-}\) + C2H4O \(\to\) C2H4O2 + Cr3+

Complete and balance the following equation:
Zn + \(NO_3^- \to\) Zn2+ + \(NH_4^+\)

Complete and balance the following equations:
Cl2 + OH- \(\to\) Cl- + ClO-

Complete and balance the following equation:
Ce3+ + \(S_2O_8^{-2} \to\) \(SO_4^{-2}\) + Ce4+

The oxidation number of carbon in CH2O is

1 mole of N2H4 loses 10 moles of electrons to form a new compound Y. assuming that all nitrogen appears in the new compound , what is the oxidation state of nitrogen in Y ? (there is no change in the oxidation state of hydrogen)

Balance the following Equations:
(i) Cu2O + H+ + \(NO_3^ - \to\) Cu2+ + NO + H2O
(ii) K4[Fe(CN)6] + H2SO4 + H2O \(\to\) K2SO4 + FeSO4 + (NH4)2SO4 + CO
(iii) C2H5OH + I2 + OH- \(\to\) CHI3 + \(HCO_3^-\) + I- + 4H2O

M is molecular weight of KMnO4. The equivalent wight of KMnO4 when it is converted into K2MnO4 is