Can someone please help me solve this.....Use the following reaction to answer the question?
Use the following reaction to answer the questions….
4Fe(s) + 3O2(g) → 2Fe2O3(g) ΔH= -1700kJ
a. How many kJ are released when 2.00g Fe react?
b. How many grams of rust form when 453kJ of energy are released?
I have all my other questions and problems solved its just this one that has me completely lost....can someone help me and explain how they got there answers? Thanks so much!
4Fe(s) + 3O2(g) → 2Fe2O3(g) ΔH= -1700kJ
a. How many kJ are released when 2.00g Fe react?
b. How many grams of rust form when 453kJ of energy are released?
I have all my other questions and problems solved its just this one that has me completely lost....can someone help me and explain how they got there answers? Thanks so much!
Best Answer - Chosen by Voters
From the equation, 4 mol of Fe will release 1700kJ of energy.
2/56 mol of Fe will release (1700/4) X (2/56)
....................................= 15.18 kJ
From the equation, 1700kJ ---------------------> 2 mol of Fe2O3 ( 2 x 160g)
.............................453kJ ----------------------> 2 x 2 x 160 x 453 /1700
......................................… = 170.54 g
2/56 mol of Fe will release (1700/4) X (2/56)
....................................= 15.18 kJ
From the equation, 1700kJ ---------------------> 2 mol of Fe2O3 ( 2 x 160g)
.............................453kJ ----------------------> 2 x 2 x 160 x 453 /1700
......................................… = 170.54 g
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