Redox Reactions...

The stoichiometric constants for the reaction $$pCu + qHNO_3 \rightarrow rCu(NO_3)_2 + sNO + tH_2O$$ p, q, r ,s and t respectively are:

For the redox reaction:

When $${{\text{K}}_{\text{2}}}{\text{C}}{{\text{r}}_{\text{2}}}{{\text{O}}_{\text{7}}}$$ is converted into $${{\text{K}}_{\text{2}}}{\text{Cr}}{{\text{O}}_4}$$, the change in oxidation number of Cr is 

Given below are the half-cell reactions:
$$Mn^{2+} + 2e^- \to Mn; E^o = -1.18V$$
$$2(Mn^{3+} + e^- \to Mn^{2+}); E^o = +1.51V$$
The $$E^o$$ for $$3Mn^{2+} \to Mn +2Mn^{3+}$$ will be:

In the electrolysis of aqueous sodium chloride solution which of the half-cell reaction will occur at the anode?

$$KMnO_4$$ acts as an oxidizing agent in acidic medium. The number of moles of $$KMnO_4$$ that will be needed to react with one mole of sulphide ions in acidic solution is:

The oxidation number and coordination number of $$M$$ in the compound, $$[M(SO_4)(NH_3)_5]$$ will be:

A metal, M forms chlorides in its +2 and +4 oxidation states. Which of the following statements about these chlorides is correct?

The magnetic moment of $$M^{x+}$$ (atomic number $$= 25$$) is $$\sqrt{15}$$ . Then, the oxidation number $$x$$ of $$M$$ is: