Redox Reactions · Chemistry · VITEEE

In the following redox reaction, what will be the sum of $x, y$, and $z$ ?

$$ \begin{aligned} x \mathrm{Cr}_2 \mathrm{O}_7^{2-}(a q) & +y \mathrm{SO}_3^{2-}(a q)+z \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Cr}^{3+}(a q)+\mathrm{SO}_4^{2-}(a q)+\mathrm{H}_2 \mathrm{O}(l) \end{aligned} $$

How many moles of $\mathrm{KMnO}_4$ are required to oxidise 1 mole of oxalic acid in acidic medium?

Ozone is quantitatively determined by bubbling it through an excess of acidic potassium iodide solution, which liberates iodine. The liberated iodine is then titrated with sodium thiosulphate solution.

If 25.0 mL of the iodine-containing solution required 20.0 mL of 0.01 M sodium thiosulphate for complete titration, calculate the number of moles of ozone that reacted.

For the given redox reaction, what will be the sum of $x, y, m$ and $n$ ?

$$\begin{aligned} x \mathrm{MnO}_4^{-}+y \mathrm{H}_2 \mathrm{C}_2 \mathrm{O}_4+z \mathrm{H}^{+} \longrightarrow m \mathrm{Mn}^{2+} + & n \mathrm{CO}_2+p \mathrm{H}_2 \mathrm{O} \end{aligned}$$

How many moles of potassium dichromate oxidises 1 mole of ferrous oxalate in acidic medium?

Ozone is determined quantitatively by first reacting it with excess of KI at a particular pH and then titrating the $\mathrm{I}_2$ thus, liberated with a suitable titrant. The pH of the reaction and the titrant used in the titration are respectively.

$$\mathrm{MnO}_4^{-}$$ is good oxidising agent in different medium changing to

$$\mathrm{MnO}_4^{-} \rightarrow \mathrm{Mn}^{2+} \rightarrow \mathrm{MnO}_4^{2-} \rightarrow \mathrm{MnO}_2 \rightarrow \mathrm{Mn}_2 \mathrm{O}_3$$

Change in oxidation number respectively are :

The standard $$E_{\text {red }}^{\circ}$$ values of $$A, B$$ and $$C$$ are $$+0.52 \mathrm{~V},-23.6 \mathrm{~V},-0.44 \mathrm{~V}$$ respectively. The order of their reducing power is