Given the following data: Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) ΔH = -462 kJ MgO(s) + 2 HCl(aq) → MgCl2(aq) + H2O(l) ΔH = -146 kJ H2(g) + 1/2 O2(g) → H2O(l) ΔH = -286 kJ what is the heat of formation of MgO? Mg(s) + 1/2 O2(g) → MgO(s)
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Step 1: Calculate the heat of formation of MgO by adding equation 1 and 3, and then subtracting equation 2. Show more…
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Using these molar enthalpy values: (1) MgO(s) + 2 HCl(aq) → MgCl2(aq) + H2O(aq) ΔH1 = -127 kJ/mol (2) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) ΔH2 = -642 kJ/mol (3) H2(g) + 1/2 O2(g) → H2O(l) ΔH3 = -285.84 kJ/mol Calculate the enthalpy of reaction 4 using Hess's Law. (4) Mg(s) + 1/2 O2(g) → MgO(s) ΔH4 = ??? kJ/mol
Pam O.
Calculate the standard enthalpy of formation of solid magnesium hydroxide (Mg(OH)2) using the following thermochemical information: 2 Mg(s) + O2(g) 2 MgO(s) H = -1203.6 kJ 2 H2O(l) 2 H2(g) + O2(g) H = +571.7 kJ Mg(OH)2(s) MgO(s) + H2O(l) H = +37.2 kJ H = ? kJ
Hitendra S.
Given that $$ \begin{aligned} \mathrm{S}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) & \longrightarrow \mathrm{SO}_{2}(\mathrm{~g}) & \Delta H &=-296.8 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{S}(\mathrm{s})+\frac{3}{2} \mathrm{O}_{2}(\mathrm{~g}) & \longrightarrow \mathrm{SO}_{3}(\mathrm{~g}) & \Delta H=-395.6 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ determine the enthalpy change for the decomposition reaction $$ 2 \mathrm{SO}_{3}(\mathrm{~g}) \longrightarrow 2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) $$
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