Question
What mass of iron can be obtained from 500.0g of Fe3O4?
I am having a hard time getting started on this question. I think I need to find the percent of iron in the compound and then multiply that by 500.0 g. But, when I tried that I got a really wonky answer.
Fe 3 55.85g/mol = 167.55/mol
O 4 16.00g/mol = 64.00g/mol
-----------
231.55g/mol
231.55g/mol = total molar mass
167.55g/mol Fe
-------------- x 100% = 72.36%
231.55g/mol
.7236% Fe x 500.0g = 361.8g
Did I get this right or do I need some major help?
I am having a hard time getting started on this question. I think I need to find the percent of iron in the compound and then multiply that by 500.0 g. But, when I tried that I got a really wonky answer.
Fe 3 55.85g/mol = 167.55/mol
O 4 16.00g/mol = 64.00g/mol
-----------
231.55g/mol
231.55g/mol = total molar mass
167.55g/mol Fe
-------------- x 100% = 72.36%
231.55g/mol
.7236% Fe x 500.0g = 361.8g
Did I get this right or do I need some major help?
Answers
Scott
looks fine