Asked by kylie
Use the following reaction to answer the questions
4Fe(s) + 3O2(g) ® 2Fe2O3(g) ÄH = -1700 kJ
How many kJ are released when 2.00 g Fe react?
How many grams of rust form when 453 kJ of energy are released?
4Fe(s) + 3O2(g) ® 2Fe2O3(g) ÄH = -1700 kJ
How many kJ are released when 2.00 g Fe react?
How many grams of rust form when 453 kJ of energy are released?
Answers
Answered by
bobpursley
Do these as a proportion..
2gramsFe/4molesFe=Energy/-1700kj
of course, convert the 4 moles to grams.
gramsrust/2molesFe2O3=-453/-1700
2gramsFe/4molesFe=Energy/-1700kj
of course, convert the 4 moles to grams.
gramsrust/2molesFe2O3=-453/-1700
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