In order to oxidize a mixture of one mole of each of $FeC_2O_4$,$Fe_2(C_2O_4)_3$,$FeSO_4$ and $Fe_2(SO_4)_3$ in acidic medium,the number of moles of $KMnO_4$ required is

Which gases are formed by the oxidation of carbon with concentrated $H_2SO_4$?

$A$ copper coin is completely covered with a gold film and is placed in dilute $HNO_3$. This will result in the formation of:

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$SrCrO_4 \downarrow + 2AcOH \text{ (Excess)} \longrightarrow Sr(AcO)_2 + H_2Cr_2O_7$

$X$ and $Y$ are the number of electrons involved,respectively,during the oxidation of $I^{-}$ to $I_{2}$ and $S^{2-}$ to $S$ by acidified $K_{2}Cr_{2}O_{7}$. The value of $X + Y$ is . . . . . . .

To measure the quantity of $MnCl_2$ dissolved in an aqueous solution,it was completely converted to $KMnO_4$ using the reaction,
$MnCl_2 + K_2S_2O_8 + H_2O \longrightarrow KMnO_4 + H_2SO_4 + HCl$ (equation not balanced).
Few drops of concentrated $HCl$ were added to this solution and gently warmed. Further,oxalic acid $(225 \ mg)$ was added in portions till the colour of the permanganate ion disappeared. The quantity of $MnCl_2$ (in $mg$) present in the initial solution is . . . . . . . . . (Atomic weights in $g \ mol^{-1}: Mn = 55, Cl = 35.5$ )