Question

Enter your answer in the provided box. An iron bar has a mass of 543 g. After the bar had been standing in air for a month, exactly one-eighth of the iron turned to rust (Fe2O3). Calculate the final mass of the iron bar and the rust.

Answer 1

? sol ? 2 ? 222222222 1) Calculate eighth ү4h4 the of mass of the bar iron has after one- undergone 22 ?? mass of fe = 5439 1/3 (543) = 475.125 g = 2) Reaction of rusting is given by 4Fe + 302 2Fe2O3

Now, the mole of iron which undergare rusting is given by mass of iron, which undergone susting molecular mass of iron Here mass of Iron, which undergone rusting is given by = 4 x 543 - 67.875g. AUSAAMAAAAAAAAIVIL molecular mass of iron = 56 So, note = 67.875 = 1.212 67.875 56 - = 1.212 from the above reaction, 4 mole of a te will give a mole of sust (Fe2O3). So, 1.212 role of fe will give 1.21 2x2 = 0.600 mole of rust (Fe2O) =

So, mass of rust (Fe2O3) - w to n к 0, xuurts алу ки of fez Oz = 0.606 x 160 27 = 96.96g So, combined mass of the iron trust sust 72 7222 = inn remain t mass of = 475.125+ 96.96 - 572.085 g (Aus)