Which of the following cannot act as an oxidizing agent?

1. $S^{2-}$

2. $B{r}_2$

3. $HS{O}_4^{-}$

4. $S{O}_3^{2-}$

Which of the following compounds has an element exhibiting two differrent oxidation states?

What is the alteration in the oxidation state of carbon in the given reaction?

\(\mathrm{{CH_4}_{(g)} + 4{Cl_2}_{(g)} \rightarrow {CCl_4}_{(l)} + 4 HCl_{(g)}}\)

The reducing ability of the metals K, Au, Zn, and Pb follows the order

${\mathrm{KMnO}}_4$ is a strong oxidising agent in acidic medium. To provide acidic medium, ${\mathrm{H}}_2{\mathrm{SO}}_4$ is used instead of HCl. This is because

1. ${\mathrm{H}}_2{\mathrm{SO}}_4$ is stronger acid than HCl
2. HCl is oxidised by ${\mathrm{KMnO}}_4$ to ${\mathrm{Cl}}_2$
3. ${\mathrm{H}}_2{\mathrm{SO}}_4$ is dibasic acid
4. Rate is faster in the presence of ${\mathrm{H}}_2{\mathrm{SO}}_4$

The element that does not show a disproportionation tendency is/are:

Which of the following statement regarding the rules to calculate the oxidation number is incorrect?

Given below are two statements: