?Consider the following reaction: \(2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{MgO}(s) \quad \Delta H=-1204 \mathrm{~kJ}\)
Chapter 5, Problem 5.43(choose chapter or problem)
Consider the following reaction:
\(2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{MgO}(s) \quad \Delta H=-1204 \mathrm{~kJ}\)
(a) Is this reaction exothermic or endothermic?
(b) Calculate the amount of heat transferred when 3.55 g of Mg(s) reacts at constant pressure.
(c) How many grams of MgO are produced during an enthalpy change of -234 kJ?
(d) How many kilojoules of heat are absorbed when 40.3 g of MgO(s) is decomposed into Mg(s) and O2(g) at constant pressure?
Text Transcription:
2 Mg(s) + O2(g) \longrightarrow 2 MgO(s) \Delta H = -1204 kJ
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