Redox Reactions

The non-metal that does not exhibit positive oxidation state is :

$\ce{Fe^{3+}}$ is reduced to $\ce{Fe^{2+}}$ by using

In dilute aqueous $\ce{H2SO4}$, the complex diaquodioxalatoferrate(II) is oxidized by $\ce{MnO4-}$. For this reaction, the ratio of the rate of change of $[\ce{H+}]$ to the rate of change of $[\ce{MnO4-}]$ is

Choose the incorrect formula out of the four compounds for an element X below :

For the reaction:
$$\ce{I- + ClO3- + H2SO4 -> Cl- + HSO4- + I2}$$
The correct statement(s) in the balanced equation is/are:

Consider the following list of reagents:

Acidified $\ce{K2Cr2O7}$, alkaline $\ce{KMnO4}$, $\ce{CuSO4}$, $\ce{H2O2}$, $\ce{Cl2}$, $\ce{O3}$, $\ce{FeCl3}$, $\ce{HNO3}$ and $\ce{Na2S2O3}$.

The total number of reagents that can oxidise aqueous iodide to iodine is

Hydrogen peroxide in its reaction with $\ce{KIO4}$ and $\ce{NH2OH}$ respectively, is acting as a

In which of the following reactions $\ce{H2O2}$ acts as a reducing agent ?

(a) $\ce{H2O2 + 2H+ + 2e- -> 2H2O}$

(b) $\ce{H2O2 - 2e- -> O2 + 2H+}$

(c) $\ce{H2O2 + 2e- -> 2OH-}$

(d) $\ce{H2O2 + 2OH- - 2e- -> O2 + 2H2O}$

The equation which is balanced and represents the correct product(s) is :

Which of the following is not formed when $\ce{H2S}$ reacts with acidic $\ce{K2Cr2O7}$ solution ?

Given

$\ce{Fe^3+(aq) + e- -> Fe^2+(aq)}$; $E^\circ=+0.77$ V

$\ce{Al^3+(aq) + 3e- -> Al(s)}$; $E^\circ=-1.66$ V

$\ce{Br2(aq) + 2e- -> 2Br-}$; $E^\circ=+1.09$ V

Considering the electrode potentials, which of the following represents the correct order of reducing power ?

Hydrogen peroxide acts both as an oxidising and as a reducing agent depending upon the nature of the reacting species. In which of the following cases $\ce{H2O2}$ acts as a reducing agent in acid medium ?

Consider the reaction :
$$\ce{H2SO3_{(aq)} + Sn^{4+}_{(aq)} + H2O_{(l)} -> Sn^{2+}_{(aq)} + HSO4^-_{(aq)} + 3H^+_{(aq)}}$$
Which of the following statements is correct ?

How many electrons are involved in the following redox reaction ?
$$\ce{Cr2O7^2- + Fe^2+ + C2O4^2- -> Cr^3+ + Fe^3+ + CO2}\ \text{(Unbalanced)}$$

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

The unbalanced chemical reactions given in List I show missing reagent or condition (?) which are provided in List II. Match List I with List II and select the correct answer using the code given below the lists:

Which ordering of compounds is according to the decreasing order of the oxidation state of nitrogen?

The reaction of white phosphorus with aqueous NaOH gives phosphine along with another phosphorus containing compound. The reaction type; the oxidation states of phosphorus in phosphine and the other product are respectively

25 mL of household bleach solution was mixed with 30 mL of 0.50 M KI and 10 mL of 4 N acetic acid. In the titration of the liberated iodine, 48 mL of 0.25 N $\ce{Na2S2O3}$ was used to reach the end point. The molarity of the household bleach solution is

For the given aqueous reactions, which of the statement(s) is (are) true?