Redox Reaction Quiz-2

The reaction, $P_4+3NaOH+3H_2O\longrightarrow3NaH_2PO_2+PH_3$ is an example of :

What volume of 0.40 M $Na_2S_2O_3$ would be required to react with the $I_2$ liberated by adding excess of KI to 50mL of 0.20 M $CuSO_4$ solution?

What is the normality of $KMnO_4$ solution to be used as an oxidant in acidic medium, which 4 contains 15.8 g of the compound in 100 mL of solution?

What volume of 1N $K_2Cr_2O_7$ solution is required to oxidise (in acidic solution) a solution containing 10 g of $FeSO_4$? (mol. wt. of $FeSO_4=152$)

A solution of $KMnO_4$ is reduced to $MnO_2$. The normality of solution is 0.6. The molarity is

Number of $K^+$ ions and moles of $K^+$ ions present in 1 litre of $\frac N5$ $KMnO_4$ acidified solution respectively are

A solution containing $2.68 \times 10^{-3}$ mol of $A^{n+}$ ions requires $1.61 \times 10^{-3}$ mol of $MnO_4^-$ for the oxidation of $A^{n+}$ to $AO_3^-$ in acidic medium. The value of n is

Number of moles of $K_2Cr_2O_7$ reduced by one mole of $Sn^{2+}$ions in acidic medium is

The equivalent weight of used as an oxidizing agent in acidic medium is (atomic weight of Ba = 137.34 and Cr = 52)

The equivalent mass of $KIO_3$ in the reaction given is $Cr(OH)_3+4OH^-+ KIO_3 \longrightarrow 2CrO^{2-}_4+ KI + 5H_2O$, (M = molecular mass of $KIO_3$)