iron(III) oxide can be reduced with carbon monoxide according to the following equation
Fe2O3(s) -->2 Fe(s) + 3 CO2 (g)
A 16.2 cL sample of CO(g) at 1.5 atm and 200*C is combined with 15.39g of Fe2O3(s)
(i)what is the limiting reactant for the reaction? justify your answer with calculations
(ii) how many moles of Fe(s) are formed in the reaction
2007-01-07 17:55:47 · 2 answers · asked by robert m 1 in Science & Mathematics ➔ Chemistry
Your equation is missing the CO on reactant side.
Balance the equation after adding the CO.
Use PV=nRT to solve for number of moles of CO (solve for n)
Then change grams of iron oxide to moles
Solve for limiting using balanced equation (ie. which one will you run out of first?)
Using your limiting, use mole-mole ratio to solve for moles of Iron (assuming 100% yield, I presume)
2007-01-07 18:07:11 · answer #1 · answered by teachbio 5 · 0⤊ 0⤋
Mr.Abdul R Baloch is Good Man
2007-01-08 02:01:03 · answer #2 · answered by a b c d e 1 · 1⤊ 0⤋