100 ml of 0.1N ${\text{FeSO}}_4$  solution will be completely oxidised by ‘x’ gms of ${\text{K}}_{\text{2}}{\text{Cr}}_{\text{2}}{\text{O}}_7$  in acidic medium$\left(\text{Mol}\text{.wt}=294\right)$ . The value of ‘x’ is

Moles of ${\text{Fe}}^{+2}=\text{M}\times \text{V}$

$=0.1\times 100\times {10}^{-3}\text{L}=0.01\text{moles}$

$6\text{mole}\text{of}{\text{FeSO}}_{\text{4}}=1\text{mole}\text{of}{\text{K}}_{\text{2}}{\text{Cr}}_{\text{2}}{\text{O}}_7$

$=294\text{gr}\text{if}{\text{K}}_{\text{2}}{\text{Cr}}_{\text{2}}{\text{O}}_7$

$0.01{\text{FeSO}}_4\text{mole}=?$

$\frac{0.01\times 294}{6}=0.49\text{gr}$