Number of moles of electrons produced per mole of \(FeCr_{2}O_{4}\) in the following redox reaction.\[FeCr_{2}O_{4}+KOH+O_{2}\rightarrow K_{2}CrO_{4}+Fe_{2}O_{3}\]

Number of moles of electorns in the reaction during formation of 1 mole of Fe_3O_4 according to the reaction Fe+H_2OtoFe_3O_4+H_2 will be :

How many moles of O_(2) will be liberated by one mole of CrO_(5) is the following reaction: CrO_(5) + H_(2) SO_(4) rarr Cr_(2) (SO_(4))_(5) + H_(2)O + O_(2)

The number of moles of Fe_(2)O_(3) formed when 0.5 moles of O_(2) and 0.5 moles of Fe are allowed to react are

The number of moles of Fe_(2)O_(3) formed when 0.5 moles of O_(2) and 0.5 moles of Fe are allowed to react are

Find the number of moles of electron exchanged in the below redox reaction for each mole of H_(2)O involved. CrI_(3) + Cl_(2) + KOH rarr K_(2)CrO_(4) + KIO_(4) + KCl + H_(2)O

How many electrons are involved in the following redox reaction? Cr_(2)O_(7)^(2-)+Fe^(2+)+C_(2)O_(4)^(2-)toCr^(3+)+Fe^(3+)+CO_(2)

In FeCr_(2)O_(4) , the oxidation numbers of Fe and Cr are :

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) ?