Consider the following reaction: 2Mg(s)+O2(g)------>2MgO(s) deltaH = -1204kJ is

Question

Consider the following reaction:

2Mg(s)+O2(g)------>2MgO(s)   deltaH = -1204kJ

is this reaction exothermic or endothermic?

   

2Mg(s)+O 2 (g)?2MgO(s)?H=?1204kJ

Consider the following reaction: 2Mg(s)+O2(g)------>2MgO(s) deltaH = -1204kJ is this reaction exothermic or endothermic? : Calculate the amount of heat transferred when 3.59g of Mg(s) { m Mg}(s) reacts at constant pressure. part C: How many grams of Mg(s) { m MgO} are produced during an enthalpy change of -239 kJ? How many kilojoules of heat are absorbed when 40.9g g g of MgO(s) is decomposed into Mg(s) { m Mg}(s) and O2g) { m {O}}_2 (g) at constant pressure? 2Mg(s)+O 2 (g)?2MgO(s)?H=?1204kJ

Explanation / Answer

The reaction is exothermic

B) Moles of Mg = 3.59 / 24.3 = 0.1477 moles

for 2 moles of Mg delta H = -1204

for 0.1477 mole

delta H = -1204 x 0.1477 / 2 = -88.94 KJ

C) Let Moles of Mg reacted = X

=> -1204 * X / 2 = -239

=> X = 0.397 moles

Moles of MgO produced = 0.397 moles

=> Mass = 0.397 x 40.3 = 16 g

D) moles of MgO = 40.9 / 40.3 = 1.015 moles

=> Heat absorbed = 1204 x 1.015 / 2 = 610.96 KJ

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