In the reaction `CrO_(5) + H_(2)SO_(4)rarr Cr_(2)(sO_(4))_(3)+H_(2)O+O_(2)`, one mole of `CrO_(5)` will liberate how many molesof `O_(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) ?

For the reaction : 4CrO_5+6H_2SO_4rarr2Cr_2(SO_4)_3+6H_2O+7O_2 . Which statement is wrong?

Balance the equation : SO_(2) + Na_(2)CrO_(4) + H_(2)SO_(4) rarr Na_(2)SO_(4) + Cr_(2)(SO_(4))_(3) + H_(2)O

Na_(2)CrO_(4)+HCl to H_(2)Cr_(2)O_(7)+Na_(2)SO_(4)

Na_(2)CrO_(4)+HCl to H_(2)Cr_(2)O_(7)+Na_(2)SO_(4)

Na_(2)CrO_(4)+HCl to H_(2)Cr_(2)O_(7)+Na_(2)SO_(4)

In the reaction, Cr_(2)O_(7)^(2-)+H_(2)O to 2CrO_(4)^(2-)+2H^(+) Cr undergoes

Can the reaction, Cr_(2)O_(7)^(2-) + H_(2)O rarr 2CrO_(4)^(2-) + 2H^(+) be regarded as a redox reaction ?

Can the reaction, Cr_(2)O_(7)^(2-) + H_(2)O rarr 2CrO_(4)^(2-) + 2H^(+) be regarded as a redox reaction ?