Method 2 - Displacement (d) The chemical equation for the displacement of copper using iron is: CuSO_(4)+Fearrow Cu+FeSO_(4) Calculate the minimum mass of iron needed to displace all of the copper from 50cm^3 of copper(II) sulfate solution. The concentration of the copper(II) sulfate solution is 80 g CuSO_(4) per dm^3 Relative atomic masses (A_(r)):O=16;S=32;Fe=56;Cu=63.5 Give your answer to 2 significant figures. Mass of iron=1.4g_(9)

For the reaction , using stoichiometric calculations we will find that every 1 moles of consume 1 mole of . So, to calculate the mass of iron we need to figure out the number moles of , then calculate the mass of .Step1: Calculate the concentration of in to : Then, Find the mass of in : Step 2: Find the molar mass of : \( M_{\mathrm{CuSO}_{4}} = 63.5 (for \, Cu) + 32 (for \, s) + (16 \times 4)(for \, O)=\mathrm{Molar} \, \mathrm{mass \, of} \, \mathrm{CuSO}_{4} \) Then , Find the number of moles of : \( Moles= \frac{Mass}{Molar Mass} = \frac{(0.08 \times 50)}{(63.5+32+16*4)} \) Step 3: Find the mass of :As we calculated before in stoichiometric relation , the numberof moles of = number of moles of . so we recalculate : \( Mass+\mathrm{Fe} = moles_{(\mathrm{Fe So_{4})} \times M_{\mathrm{Fe}} \)