In acidic medium,potassium dichromate acts as an oxidant according to the equation,$Cr_2O_7^{2-} + 14H^{+} + 6e^- \to 2Cr^{3+} + 7H_2O$. What is the equivalent weight of $K_2Cr_2O_7$? (Molecular weight $= M$)

How many electrons are lost in the following transformation?
$3Fe + 4H_2O \to Fe_3O_4 + 4H_2$

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$Ca_{(s)} + 2H_2O_{(l)} \xrightarrow{R.T.} Ca(OH)_{2(aq)} + H_{2(g)} \uparrow$

In the reaction between $KI$ and acidic potassium dichromate solution,the oxidation state of chromium in the final product is ........

If the number of moles of $Fe^{2+}$ ions oxidized by one mole of acidified $MnO_4^{-}$ is $x$, the number of moles of $Fe^{2+}$ ions oxidized by one mole of acidified $Cr_2O_7^{2-}$ is:

Consider the following redox reaction taking place in acidic medium: $BH_{4}^{-}(aq) + ClO_{3}^{-}(aq) \rightarrow H_{2}BO_{3}^{-}(aq) + Cl^{-}(aq)$. If the Nernst equation for the above balanced reaction is $E_{cell} = E_{cell}^{o} - \frac{RT}{nF} \ln Q$, then the value of $n$ is . . . . . . . (Nearest integer)