Balancing redox reactions

500 mL of 0.2 M $\ce{MnO4-}$ solution in basic medium when mixed with 500 mL of 1.5 M KI solution, oxidises iodide ions to liberate molecular iodine. This liberated iodine is then titrated with a standard $x$ M thiosulphate solution in presence of starch till the end point. If 300 mL of thiosulphate was consumed, then the value of $x$ is ________.

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

An aqueous solution of hydrazine ($\ce{N2H4}$) is electrochemically oxidized by $\ce{O2}$, thereby releasing chemical energy in the form of electrical energy. One of the products generated from the electrochemical reaction is $\ce{N2(g)}$.

Choose the correct statement(s) about the above process

The number of moles of potassium iodide required to produce two moles of P is _____.

$\ce{H2S}$ (5 moles) reacts completely with acidified aqueous potassium permanganate solution. In this reaction, the number of moles of water produced is $\mathbf x$, and the number of moles of electrons involved is $\mathbf y$. The value of $(\mathbf x + \mathbf y)$ is _____.

Which one of the following reactions indicates the reducing ability of hydrogen peroxide in basic medium ?

The reaction of $\mathrm{H_2O_2}$ with potassium permanganate in acidic medium leads to the formation of mainly :

In neutral or alkaline solution, $\mathrm{MnO_4^-}$ oxidises thiosulphate to :

The reaction of sulphur in alkaline medium is given below :

$\mathrm{S_{8(s)}+a\,OH^-_{(aq)}\to b\,S^{2-}_{(aq)}+c\,S_2O_3^{2-}{}_{(aq)}+d\,H_2O_{(l)}}$

The values of 'a' is _______. (Integer answer)

In the chemical reaction between stoichiometric quantities of $\ce{KMnO4}$ and KI in weakly basic solution, what is the number of moles of $\ce{I2}$ released for 4 moles of $\ce{KMnO4}$ consumed?

Fusion of $\ce{MnO2}$ with KOH in presence of $\ce{O2}$ produces a salt W. Alkaline solution of W upon electrolytic oxidation yields another salt X. The manganese containing ions present in W and X, respectively, are Y and Z. Correct statement(s) is(are)

The amount of water produced (in g) in the oxidation of 1 mole of rhombic sulphur by conc. $\ce{HNO3}$ to a compound with the highest oxidation state of sulphur is ______

(Given data: Molar mass of water = 18 g mol⁻¹)

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

The reaction of zinc with dilute and concentrated nitric acid, respectively, produces :

$\ce{Fe^{3+}}$ 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

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

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 ?

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