Consider the following heat changes in the oxidation of magnesium and iron. Reaction involved: (i) (mathrm{Mg}+frac{1}{2} mathrm{O}_{2}=mathrm{MgO}

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Consider the following heat changes in the oxidation of magnesium and iron.

Reaction involved:

(i) $\mathrm{Mg}+\frac{1}{2} \mathrm{O}_{2}=\mathrm{MgO} \quad \Delta H=-602.06 \mathrm{~kJ} / \mathrm{mol}$

(ii) $2 \mathrm{Fe}+\frac{3}{2} \mathrm{O}_{2}=\mathrm{Fe}_{2} \mathrm{O}_{3} \quad \Delta H=-810.14 \mathrm{~kJ} / \mathrm{mol}$

Calculate the heat produced in the reaction.

\[ 3 \mathrm{Mg}+\mathrm{Fe}_{2} \mathrm{O}_{3}=3 \mathrm{MgO}+2 \mathrm{Fe} \]

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Introduction To Chemical Engineering Thermodynamics

ISBN: 9788120348974

2nd Edition

Authors: HALDER

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Question Posted: May 02, 2024 01:47 AM

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Consider the following heat changes in the oxidation of magnesium and iron. Reaction involved: (i) (mathrm{Mg}+frac{1}{2} mathrm{O}_{2}=mathrm{MgO}

Question:

Step by Step Answer:

Multiplying reaction i by 3 we get iii 3 mathrmMgfrac32 mathrmO23 mathrmMgO Delt...View the full answer

Introduction To Chemical Engineering Thermodynamics

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