A 0.2755 g sample of an iron-carbon alloy was treated with 12.0 mL of a HCl solution. The alloy sample produced 74.5 mL of H2 gas at 2 atm and 25.0 oC. Determine the molarity of the HCl solution. Determine the mass % of iron in the alloy. 2 Fe + 6 HCl T 2 FeCl3 + 3 H2
2 Fe + 6 HCl--->FeCl3 + 3 H2
m = 0.2755
PV = nRT
n = PV/(RT) = 2*74.5/1000 / (0.082*298) = 0.0060975609 mol of H2
find moles of Hcl
since ratio is 3:6
then
0.0060975609*2 = 0.0121951218mol of HCl
then
M = mol/V = 0.0121951218/(12*10^-3) = 1.0162 M of HCl
c)
% mass of Fe
find moles of Fe
since ratio is 3:2 then 2/3*0.0060975609 = 0.0040650406 mol of Fe
mass = mol*MW = 0.0040650406*55.5 = 0.2256097533 g of Fe
% mass = Fe / total * 100 = 0.2256097533/0.2755 *100 = 81.8910% of Fe
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