Question #27fd7
1 Answer
Explanation:
The idea here is that you need to use the molar mass of ferrous oxide,
Once you know how many grams of iron you get per
So, ferrous oxide has a molar mass of
You also know that one mole of ferrous oxide contains
- one mole of iron,
#1 xx "Fe"# - one mole of oxygen,
#1 xx "O"#
Elemental iron has a molar mass of
This means that every
#"% Fe" = (55.845 color(red)(cancel(color(black)("g"))))/(71.844color(red)(cancel(color(black)("g")))) xx 100 = "77.73% Fe"#
So, if every
#5 color(red)(cancel(color(black)("g FeO"))) * "77.73 g Fe"/(100color(red)(cancel(color(black)("g FeO")))) = "3.8865 g Fe"#
Rounded to one sig fig, the number of sig figs you have for the mass of ferrous oxide, the answer will be
#"mass of Fe" = color(green)(|bar(ul(color(white)(a/a)"4 g"color(white)(a/a)|)))#