Use the values you measured for Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ΔH°1: -452kJ, and MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) ΔH°2: -133kJ, with the known ΔH°3 = ΔH°f(H2O, l) = –286 kJ/mol, to find your experimental ΔH°f(MgO), as: [f MgO] Mg(s) + ½O2(g) → MgO(s) ΔH°f(MgO) = ΔH°1 – ΔH°2 + ΔH°3 = ______ kJ/mol
Use the values you measured for Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ΔH°1: -452kJ, and MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) ΔH°2: -133kJ, with the known ΔH°3 = ΔH°f(H2O, l) = –286 kJ/mol, to find your experimental ΔH°f(MgO), as: [f MgO] Mg(s) + ½O2(g) → MgO(s) ΔH°f(MgO) = ΔH°1 – ΔH°2 + ΔH°3 = ______ kJ/mol
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section5.5: Enthalpy Changes For Chemical Reactions
Problem 1RC: 1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s), ∆rH° = 181.6 kJ/mol-rxn. What is the enthalpy change...
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Use the values you measured for Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) ΔH°1: -452kJ, and MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) ΔH°2: -133kJ, with the known ΔH°3 = ΔH°f(H2O, l) = –286 kJ/mol, to find your experimental ΔH°f(MgO), as:
[f MgO] Mg(s) + ½O2(g) → MgO(s) ΔH°f(MgO) = ΔH°1 – ΔH°2 + ΔH°3 = ______ kJ/mol
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