How manay grams of K_(2)Cr_(2)O_(7) are required ot oxidise Fe^(2+) present in 15.2 g ofFeSO_(4) to Fe^(3+) if the reaction is carried out in an acidic medium ?

How manay grams of K_(2)Cr_(2)O_(7) are required ot oxidise Fe^(2+) pr

1.	How manay grams of K_(2)Cr_(2)O_(7) are required ot oxidise Fe^(2+) present in 15.2 g ofFeSO_(4) to Fe^(3+) if the reaction is carried out in an acidic medium ?
Answer» SOLUTION :The balanced chemical equation for the redox reaction is `K_(2)Cr_(2)O_(7)+6FeSO_(4)+7H_(2)SO_(45)rarrK_(2)SO_(4)+Cr_(2)(SO_(4))_(3)+7H_(2)` From the balanced equation it is clear that 6 Moles of `FeSO_(4)=1 "Mole of" K_(2)Cr_(2)O_(7) or 6xx152 g"for" FeSO_(4)` are oxidised by `K_(2)Cr_(2)O_(7)=294` g 152 g of `FeSO_(4)` are oxidised by `K_(2)Cr_(2)O_(7)=(294)/(6xx152)xx15.2=4.9 g`