ch.6.5.the overall reaction in a commercial heat pack can be represented as 4Fe(s)+3O2(g)->2Fe2O3(s) H = -1652kJa. how much heat is released when 4.80 moles of iron are reacted with excess O2?b. how much heat is released when 1.00 mole of Fe2O3 is produced ?c. how much heat is released when 1.00 g iron is reacted with excess O2?d. how much heat is released when 10.4 g Fe and 1.80 g O2 are reacted?

As per guidelines if multipart question , first three (a, b and c) are allowed t answer , please post seperately Given reaction is 4 Fe(s) + 3 O2 (g) --> 2 Fe2O3 (s) H = -1652kJ as per equation If 4 mole Fe reacted →released 1652 KJ energy when 2 mole of Fe2 O3 is produced →released 1652 KJ energy a. 4 mole Fe reacted →released 1652 KJ energy 4.8 mole Fe reacted →release ? energy Amount of energy released = - (4.8 mole Fe/ 2 mol Fe ) x 1652 KJ = - 1982.4 KJ b. Amount of energy released = - (1 mole Fe2O3 / 2 mol Fe2O3 ) x 1652 KJ = - 826 KJ c. 4 mole Fe = 4 x 55.845 g/mol = 223.4 g reacted →released 1652 KJ energy 1 g Fe reacted →release ? energy Amount of energy released = - ( 1 g Fe/ 223.4 g Fe ) x 1652 KJ = - 7.39 KJ

Answered: the overall reaction in a commercial…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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ch.6.5.

the overall reaction in a commercial heat pack can be represented as

4Fe(s)+3O₂(g)->2Fe₂O₃(s) H = -1652kJ

a. how much heat is released when 4.80 moles of iron are reacted with excess O₂?

b. how much heat is released when 1.00 mole of Fe₂O₃ is produced ?

c. how much heat is released when 1.00 g iron is reacted with excess O₂?

d. how much heat is released when 10.4 g Fe and 1.80 g O₂ are reacted?

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