In a balanced redox reaction net gain of electron (s) is equal to net loss of electrons (s).`n_("factor")` is a reaction specific parameter and for intermolecular redox reaction n-factor of oxidising reducing agent is the no. of moles of electron gained /lost by one mole of compound.
The `n_("factor")` of KI in the following reaction is :
`CuSO_(4)+KI to Cu_(2)I_(2)+K_(2)SO_(4)+I_(2)`

In a balanced redox reaction net gain of electron (s) is equal to net loss of electrons (s). n_("factor") is a reaction specific parameter and for intermolecular redox reaction n-factor of oxidising reducing agent is the no. of moles of electron gained /lost by one mole of compound. Consider the following reaction: CrO_(5)+H_(2)SO_(4) to Cr_(2)(SO_(4))_(3)+H_(2)O+O_(2) One mole of CrO_(5) will liberate how many moles of O_(2) ?

Which is the reducing agent in the following reaction 2CuSO_(4)+4KItoCu_(2)I_(2)+I_(2)+2K_(2)SO_(4) ?

Find out the given reaction in a redox reaction? 2CuSO_4 + 4Kl rarr Cu_2I_2 + 2K_2SO_4 + I_2

Complete the given redox reaction H_(2)S+K_(2)CrO_(4)+H_(2)SO_(4) rarr

Identify oxidising are reducing agents in the following reactions : (i) 2H_(2)S +SO_(2) to 3S +2H_(2)O (ii) Zn + CuSO_(4) to ZnSO_(4) +Cu

Find the number of moles of KMnO_(4) needed to oxidise one mole Cu_(2)S in acidic medium. The reaction is KMnO_(4) + Cu_(2)S rarr M n^(2+) + Cu^(2+) + SO_(2)

The standard emf of a galvanic cell involving 2 moles of electrons in its redox reaction is 0.59 V . The equilibrium constant for the redox reaction of the cell is