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)`

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) ?

The equivalent weight of H_(2)SO_(4) in the following reaction is Na_(2)Cr_(2)O_(7)+3SO_(2)+H_(2)SO_(4)rarr3Na_(2)SO_(4)+Cr_(2)(SO_(4))_(3)+H_(2)O

The equivalent weight of H_(2)SO_(4) in the following reaction is Na_(2)Cr_(2)O_(7)+3SO_(2)+H_(2)SO_(4)rarr3Na_(2)SO_(4)+Cr_(2)(SO_(4))_(3)+H_(2)O

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

How many moles of electrons are needed for the reduction of each mole of Cr in the reaction, CrO_5+H_2​SO_4 rarr Cr_ 2(SO _4 )_ 3+H_2O+O_2 ​

Find out the statement which is not correct for the following reaction 4CrO_5 + 6H_2SO_4 -→2 Cr_2(SO_4)3 + 6H_2O + 7O_2

Which of the following statements is/are correct about the reaction. 4CrO_(5)+6H_(2)SO_(4)to2Cr_(2)(SO_(4))_(3)+6H_(2)O+7O_(2)

Which of the following statements is/are correct about the reaction. 4CrO_(5)+6H_(2)SO_(4)to2Cr_(2)(SO_(4))_(3)+6H_(2)O+7O_(2)