How much heat is released when 0.250 kg of iron rusts? 4 Fe (s)+ 3 O2 (g) ? 2 Fe2O3 (s) ?H = -1.65 x 103 kJ

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Tod ThielLv2

17 Dec 2019

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Related questions

Given the reaction: 4 Fe (s) + 3 O2 (g)--> 2Fe2O3 (s) ?H= -1.65x 10^3 kJ

use stoichiometry to solve:

How many mol of O2 are required to form 3.20 mol Fe2O3 and how muchheat is exchanged when 14.3 kg of iron rusts?

please show step by step instructions so I can better understandand work on other problems. thank you
Fe=55.85
O=16.00

The overall reaction in commercial heat packs can be represented asthe reaction below.
4 Fe(s) + 3 O2(g) ? 2 Fe2O3(s), ?H = -1652 kJ
(a) How much heat is released when 4.13 mol iron is reacted withexcess O2?
___kJ

(b) How much heat is released when 1.46 mol Fe2O3 isproduced?
___kJ

(c) How much heat is released when 1.00 g iron is reacted withexcess O2?
___kJ

(d) How much heat is released when 14.70 g Fe and 2.22 g O2 arereacted?
___kJ