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
Added by Richard J.
Step 1
First, we need to rearrange the given equations to match the formation of Mg(OH)2(s) from its elements, which are Mg(s), H2(g), and O2(g). Show more…
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Determine the enthalpy of formation of MgO from the following. (***reminder: you may have to rearrange the equations!!!) Round answer to the nearest whole number. Mg(s) + 2H+(aq) → Mg2+(aq) + H2(g) ΔH = -229 MgO(s) + 2H+(aq) → Mg2+(aq) + H2O(l) ΔH = -74 H2(g) + 1/2O2(g) → H2O(g) ΔH = -286 Mg(s) + 1/2O2(g) → MgO(s) ΔH = ???
Adi S.
Using these molar enthalpy values: (1) MgO(s) + 2 HCl(aq) → MgCl2(aq) + H2O(aq) ΔH1 = -134 kJ/mol (2) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) ΔH2 = -587 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
Luke M.
The enthalpy of formation of magnesium oxide, $\mathrm{MgO}(\mathrm{s}),$ is $-601827 \mathrm{kJ} / \mathrm{kmol}$ at $25^{\circ} \mathrm{C}$. The melting point of magnesium oxide is approximately $3000 \mathrm{K},$ and the increase in enthalpy between 298 and $3000 \mathrm{K}$ is $128449 \mathrm{kJ} / \mathrm{kmol}$. The enthalpy of sublimation at $3000 \mathrm{K}$ is estimated at 418000 $\mathrm{kJ} / \mathrm{kmol}$, and the specific heat of magnesium oxide vapor above $3000 \mathrm{K}$ is estimated at 37.24 $\mathrm{kJ} / \mathrm{kmol} \mathrm{K}.$
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